(I already have part A but still still include it anyways so you can use its data to solve for parts B and C.
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction:
ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants)
Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, ΔG∘. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction:
ΔG∘=ΔH∘−TΔS∘
where T is standard temperature, 298 K.
Part A
Part complete
Calculate the standard enthalpy change for the reaction
2A+B⇌2C+2D
where the heats of formation are given in the following table:
Substance | ΔH∘f (kJ/mol) |
A | -261 |
B | -425 |
C | 175 |
D | -491 |
Express your answer in kilojoules.
ΔH∘rxn = 315 kJ
Part B
For the reaction given in Part A, how much heat is absorbed when 3.30 mol of A reacts?
Express your answer numerically in kilojoules.
Part C
For the reaction given in Part A, ΔS∘rxn is 41.0 J/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxn?
Express your answer numerically in kilojoules.
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