Equilibrium ICE Table - Questions

The Equilibrium ICE Table Concept Builder is comprised of 48 questions. The questions are organized into 12 different Question Groups and spread across three difficulty levels. Questions in the same group are rather similar to one another; they include the same reaction and the same general set of given information (though different numbers). The Concept Builder is coded to select at random a question from each group until a student is successful with that group of questions.

There are three difficulty levels that can be engaged in through the Concept Builder. Those three levels are differentiated as follows:
 

• Apprentice Difficulty Level: Question Groups 1-4 ... Initial concentrations for all reactants and products are given. The equilibrium concentration is given the reactant. The reaction involves coefficients of 1 such that the equilibrium expression does not have any powers other than 1.
• Master Difficulty Level: Question Groups 5-8 ... Initial concentrations for all reactants and products are given. The equilibrium concentration is given for one of the products (the one that has a coefficient of 1). The reaction involves coefficients other than 1 such that the equilibrium expression has powers other than 1.
• Wizard Difficulty Level: Question Groups 9-12 ... The container volume and the initial number of moles for all reactants and producs are given. The # of moles is given for one of the products (for which the coefficient is not 1). The reaction involves coefficients other than 1 such that the equilibrium expression has powers other than 1.

The questions from each group are shown below. Teachers are encouraged to view the questions in order to judge which activities are most appropriate for their classes. We recommend providing students two or more options. 

The Physics Classroom grants teachers and other users the right to print these questions for private use. Users are also granted the right to copy the text and modify it for their own use. However, this document should not be uploaded to other servers for distribution to and/or display by others. The Physics Classroom website should remain the only website or server from which the document is distributed or displayed. We also provide a PDF that teachers can use under the same conditions. We have included a link to the PDF near the bottom of this page.

 

Equilibrium ICE Tables

 
Apprentice Difficulty Level
Question Group 1
Question 1
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.00 M PCl₅. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.40 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eqis 0.40 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 

 
Question 2
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 3.00 M PCl₅. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eqis 0.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 
 

 
Question 3
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.80 M PCl₅. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eqis 0.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 
 

 
Question 4
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.6 M PCl₅. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eqis 0.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 
 
 
 

 
Question Group 2
Question 5
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.00 M Cl₂ and 2.00 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.60 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 0.60 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 6
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.50 M Cl₂ and 2.50 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.70 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 0.70 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 

 
Question 7
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.80 M Cl₂ and 2.80 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 0.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 

 
Question 8
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.90 M Cl₂ and 1.90 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.40 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 0.40 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 3
Question 9
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.00 M PCl₅, 1.80 M Cl₂ and 1.80 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.1.20 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.20 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 10
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.60 M PCl₅, 2.00 M Cl₂ and 2.00 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.1.20 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.20 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 

 
Question 11
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 2.40 M PCl₅, 2.80 M Cl₂ and 2.80 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.1.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 

 
Question 12
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.50 M PCl₅, 1.80 M Cl₂ and 1.80 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 0.0.90 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 0.90 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 4
Question 13
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.00 M PCl₅, 2.80 M Cl₂ and 3.00 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 1.40 M.
   
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.40 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 14
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 0.80 M PCl₅, 2.60 M Cl₂and 3.20 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 1.20 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.20 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 15
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 0.90 M PCl₅, 3.6 M Cl₂ and 2.50 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 1.40 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.40 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 16
Consider the reversible system:  PCl_5(g)     ⇄      Cl_2(g)    +    PCl_3(g) 
A container is filled with 1.00 M PCl₅, 3.4 M Cl₂and 2.80 M PCl₃. The reaction proceeds to equilibrium. The equilibrium concentration of PCl₅ is 1.60 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [PCl₅]_eq is 1.60 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
 
Master Difficulty Level
Question Group 5
Question 17
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 6.00 mol of N₂and 5.40 mol of H₂. Once equilibrium is reached, there are 4.80 mole of N₂ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 2.40 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 18
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 3.20 M N₂and 3.20 M H₂. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 2.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 2.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 

Question 19
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.20 M N₂and 2.20 M H₂. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 20
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 1.80 M N₂and 1.80 M H₂. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
 
 
 
Question Group 6
Question 21
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.50 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 0.60 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 0.60 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
 
 
 
Question 22
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.00 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 0.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 0.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
 
 
Question 23
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 1.80 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 0.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 0.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
 
 
 
Question 24
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 3.00 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 0.60 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eqis 0.60 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
 
Question Group 7
Question 25
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.50 M N₂, 3.50 M H₂, and 3.00 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 2.00 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 2.00 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 26
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.40 M N₂, 2.80 M H₂, and 1.40 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 2.00 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 2.00 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 27
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 3.00 M N₂, 2.80 M H₂, and 1.40 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 2.50 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 2.50 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 28
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 2.10 M N₂, 2.60 M H₂, and 0.50 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.60 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.60 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 8
Question 29
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 1.40 M N₂, 0.80 M H₂, and 3.40 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.80 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.80 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 30
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 0.80 M N₂, 0.80 M H₂, and 3.60 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.30 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.30 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 31
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 0.40 M N₂, 0.60 M H₂, and 3.60 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.00 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.00 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 32
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A container is filled with 1.00 M N₂, 1.00 M H₂, and 2.80 M NH₃. The reaction proceeds to equilibrium. The equilibrium concentration of N₂ is 1.30 M.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use the number pad to complete. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know [N₂]_eq is 1.30 M, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 
Wizard Difficulty Level
Question Group 9
Question 33
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 6.00 mol of N₂ and 5.40 mol of H₂. Once equilibrium is reached, there are 2.40 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 2.40 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 34
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 4.00-L container is filled with 4.80 mol of N₂ and 6.00 mol of H₂. Once equilibrium is reached, there are 1.60 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 1.60 mol of NH₃ per 4.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 35
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 1.50-L container is filled with 4.50 mol of N₂ and 7.50 mol of H₂. Once equilibrium is reached, there are 3.00 mole of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 3.00 mol of NH₃ per 1.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 36
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 3.20 mol of N₂ and 4.50 mol of H₂. Once equilibrium is reached, there are 2.00 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 2.00 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 10
Question 37
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 1.50-L container is filled with 7.50 mol of NH₃. Once equilibrium is reached, there are 4.50 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 4.50 mol of NH₃ per 1.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 38
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 8.00 mol of NH₃. Once equilibrium is reached, there are 4.80 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 4.80 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 39
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 6.00 mol of NH₃. Once equilibrium is reached, there are 3.20 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 3.20 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 40
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 2.20 mol of NH₃. Once equilibrium is reached, there are 1.40 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 1.40 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 11
Question 41
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 1.60 mol of N₂, 1.80 mol of H₂, and 0.70 mol of NH₃. Once equilibrium is reached, there are 1.30 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 1.30 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 42
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 1.80 mol of N₂, 2.10 mol of H₂, and 1.75 mol of NH₃. Once equilibrium is reached, there are 2.25 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 2.25 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 43
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 3.20 mol of N₂, 4.00 mol of H₂, and 1.40 mol of NH₃. Once equilibrium is reached, there are 2.60 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 2.60 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 44
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 4.80 mol of N₂, 5.20 mol of H₂, and 0.60 mol of NH₃. Once equilibrium is reached, there are 2.60 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 2.60 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question Group 12
Question 45
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 2.40 mol of N₂, 2.40 mol of H₂, and 8.00 mol of NH₃. Once equilibrium is reached, there are 6.40 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 6.40 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 46
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 2.00-L container is filled with 2.00 mol of N₂, 2.00 mol of H₂, and 7.20 mol of NH₃. Once equilibrium is reached, there are 5.60 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 5.60 mol of NH₃ per 2.00 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 47
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 0.30 mol of N₂, 0.40 mol of H₂, and 1.60 mol of NH₃. Once equilibrium is reached, there are 1.20 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 1.20 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.
 
 

 
Question 48
Consider the reversible system:      N_2(g)    +    3 H_2(g)      ⇄      2 NH_3(g)
A 0.50-L container is filled with 0.50 mol of N₂, 0.50 mol of H₂, and 1.40 mol of NH₃. Once equilibrium is reached, there are 1.10 mol of NH₃ present.
 

 
Identify the K expression for this reaction.
Tap on a table cell in the first row (Initial concentration) of the ICE Table and use volume and # of moles to calculate the [ ]. Use the number pad to enter concentration values. 
Tap on a table cell in the second row (Change in concentration) and use the symbol pad to complete. 
So the third row (Equilibrium concentration) of the ICE Table is the initial concentration plus the change in concentration (i.e., the sum of the first two rows).
Given that we know there are 1.10 mol of NH₃ per 0.50 L at equilibrium, determine the value of x.
Now that you know x, use the expressions for the equilibrium [ ] (E row of ICE table) to determine the value of all equilibrium [ ]s.
Calculate the value of K. For best results, enter the answer to at least 3 significant digits.