Use a ∆H value or a thermochemical equation to determine the amount of heat released or required when given the moles of reactant or product involved in the reaction. Includes 6 problems.
Consider the balanced chemical equation and enthalpy change value for the synthesis of xenon tetrafluoride from its elements:
Xe + 2 F2 ====> XeF4
∆H = -251 kJ
How much energy will be released by the reaction of 3.0 moles of xenon?
Energy Released
kJ
How much energy will be released by the reaction of 10.0 moles of xenon?
How much energy will be released by the reaction of 0.20 moles of xenon?
Consider the balanced chemical equation and enthalpy change value for the synthesis of sulfur trioxide from its elements:
2 S + 3 O2 → 2 SO3
∆H = 790 kJ
How much energy will be required for the reaction of 10.0 moles of sulfur?
Energy Required
How much energy will be required for the reaction of 18.0 moles of sulfur?
How much energy will be required for the reaction of 7.0 moles of sulfur?
The thermochemical equation for the industrial production of sulfuric acid (H2SO4) from sulfur trioxide and water is shown below.
SO3 + H2O → H2SO4 + 227 kJ
Determine the amount of energy released when 33.0 moles of H2SO4 are produced.
Determine the amount of energy released when 84.7 moles of SO3 are reacted.
The thermochemical equation describing the reaction that takes place in a canned heating system is
2 CH3OH + 3 O2 → 2 CO2 + 4 H2O + 1199 kJ
How much energy is released by the combustion of 1.08 moles of methanol (CH3OH)?
Old-fashioned camera flash bulbs consisted of magnesium metal that would ignite with oxygen to produce a flash of energy. The balanced chemical equation and associated enthalpy change are …
2 Mg + O2 → 2 MgO
∆H = -1204 kJ
How much energy is released by the reaction of 0.0230 moles of magnesium?
Consider the balanced chemical equation and associated enthalpy change for the synthesis of ammonia (NH3) from its elements.
N2 + 3 H2 → 2 NH3
∆H = -2.7 kJ
How much energy is released when 492 moles of ammonia are produced?