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Set ST12: Stoichiometry and ICE Tables

Problem
Points
0/6
0/8
0/6
0/8
0/6
0/8
Total Score
0/42
Percentage
0 %
Assignment Overview

Use an ICE Table (Initial-Change-Ending) to analyze a limiting/excess reactant problem. 

 1. ST12Q1
Points: 0/6

Consider the balanced chemical equation for the synthesis of hydrochloric acid from its elements:

H2 + Cl2 → 2 HCl

The two reactants are initially mixed in the following amounts:

  3.08 moles of H2

  2.05 moles of Cl2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Change in Moles H2:

    mol

  2. Change in Moles Cl2:

    mol

  3. Change in Moles HCl:

    mol

  4. Ending Moles H2:

    mol

  5. Ending Moles Cl2:

    mol

  6. Ending Moles HCl:

    mol

 2. ST12Q2
Points: 0/8

Consider the balanced chemical equation for the synthesis of hydrochloric acid from its elements:

H2 + Cl2 → 2 HCl

The two reactants are initially mixed in the following amounts:

   7.26 g of H2

   78.4 g of Cl2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Initial Moles H2:

    mol

  2. Initial Moles Cl2:

    mol

  3. Change in Moles H2:

    mol

  4. Change in Moles Cl2:

    mol

  5. Change in Moles HCl:

    mol

  6. Ending Moles H2:

    mol

  7. Ending Moles Cl2:

    mol

  8. Ending Moles HCl:

    mol

 3. ST12Q3
Points: 0/6

Consider the balanced chemical equation for the synthesis of water from its elements:

2 H2 + O2 → 2 H2O

The two reactants are initially mixed in the following amounts:

6.30 moles of H2

4.10 moles of O2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Change in Moles H2:

    mol

  2. Change in Moles O2:

    mol

  3. Change in Moles H2O:

    mol

  4. Ending Moles H2:

    mol

  5. Ending Moles O2:

    mol

  6. Ending Moles H2O:

    mol

 4. ST12Q4
Points: 0/8

Consider the balanced chemical equation for the synthesis of water from its elements:

2 H2 + O2 → 2 H2O

The two reactants are initially mixed in the following amounts:

   13.7 g of H2

   69.8 g of O2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Initial Moles H2:

    mol

  2. Initial Moles O2:

    mol

  3. Change in Moles H2:

    mol

  4. Change in Moles O2:

    mol

  5. Change in Moles H2O:

    mol

  6. Ending Moles H2:

    mol

  7. Ending Moles O2:

    mol

  8. Ending Moles H2O:

    mol

 5. ST12Q5V2
Points: 0/6

Consider the balanced chemical equation for the synthesis of ammonia from its elements:

N2 + 3 H2 → 2 NH3

The two reactants are initially mixed in the following amounts:

   14.4 moles of N2

   36.7 moles of H2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Change in Moles N2:

    mol

  2. Change in Moles H2:

    mol

  3. Change in Moles NH3:

    mol

  4. Ending Moles N2:

    mol

  5. Ending Moles H2:

    mol

  6. Ending Moles NH3:

    mol

 6. ST12Q6
Points: 0/8

Consider the balanced chemical equation for the synthesis of ammonia from its elements:

N2 + 3 H2 → 2 NH3

The two reactants are initially mixed in the following amounts:

  39.1 g of N2

  16.2 g of H2

Determine the limiting and excess reactants and use this information to complete the cells of the following table. Enter all values as positive values.

  1. Initial Moles N2:

    mol

  2. Initial Moles H2:

    mol

  3. Change in Moles N2:

    mol

  4. Change in Moles H2:

    mol

  5. Change in Moles NH3:

    mol

  6. Ending Moles N2:

    mol

  7. Ending Moles H2:

    mol

  8. Ending Moles NH3:

    mol


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