Question

In: Chemistry

Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn,...

Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T. (Assume that all reactants and products are in their standard states.)

Part A ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer.

Part B ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=860K Express your answer as an integer.

Part C ΔH∘rxn=84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer.

Part D ΔH∘rxn=−84kJ, ΔS∘rxn=157J/K, T=398K Express your answer as an integer.

Solutions

Expert Solution

A)

deltaH = -84.0KJ/mol

deltaS = -157J/mol.K

= -0.157 KJ/mol.K

T = 302 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = -84.0 - 302.0 * -0.157

deltaG = -36.586 KJ/mol

Answer: -37 KJ/mol

B)

deltaH = -84.0KJ/mol

deltaS = -157J/mol.K

= -0.157 KJ/mol.K

T = 860 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = -84.0 - 860.0 * -0.157

deltaG = 51.02 KJ/mol

Answer: 51 KJ/mol

C)

deltaH = 84.0KJ/mol

deltaS = -157J/mol.K

= -0.157 KJ/mol.K

T = 302 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = 84.0 - 302.0 * -0.157

deltaG = 131.414 KJ/mol

Answer: 131 KJ/mol

D)

deltaH = -84.0KJ/mol

deltaS = 157J/mol.K

= 0.157 KJ/mol.K

T = 398 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = -84.0 - 398.0 * 0.157

deltaG = -146.486 KJ/mol

Answer: -146 KJ/mol

queen_honey_blossom answered 2 years ago
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