Question 1

Calculate ?S°S1U1B1rxnS1U1B0 for the following reaction.The S° for each species is shown below the reaction.
CS1U1B12S1U1B0HS1U1B12S1U1B0(g)+ HS1U1B12S1U1B0(g)? CS1U1B12S1U1B0HS1U1B14S1U1B0(g)
S°(J/mol?K)200.9 130.7 219.3

Accepted Answer

A) +112.3 J/K 
B) +550.9 J/K 
C) -112.3 J/K 
D) +337.1 J/K 
E) -550.9 J/K

Question 2

Determine the equilibrium constant for the following reaction at 298 K.
Cl(g)+ O3(g)→ ClO(g)+ O2(g)ΔG° = -34.5 kJ

Accepted Answer

A) 5.66 × 105 
B) 0.986 
C) 8.96 × 10-7 
D) 4.98 × 10-4 
E) 1.12 × 106

Question 3

What can you conclude about ΔG°rxn for the reaction at 25°C?
H2(g)+ Br2(g)⇌ 2 HBr(g)K = 2 × 1019

Accepted Answer

A) ΔG°rxn rxn > 0 
C) ΔG°rxn = 0 
D) There is not enough information to determine the sign or magnitude of ΔG°rxn.

Exam 17: Free Energy and Thermodynamics

Calculate ?S°_rxn for the following reaction.The S° for each species is shown below the reaction. C₂H₂(g) + H₂(g) ? C₂H₄(g) S°(J/mol?K) 200.9 130.7 219.3

Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG° = -34.5 kJ

What can you conclude about ΔG°_rxnfor the reaction at 25°C? H₂(g) + Br₂(g) ⇌ 2 HBr(g) K = 2 × 10¹⁹

Exam 17: Free Energy and Thermodynamics

Calculate ?S°rxn for the following reaction.The S° for each species is shown below the reaction. C2H2(g) + H2(g) ? C2H4(g) S°(J/mol?K) 200.9 130.7 219.3

Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O3(g) → ClO(g) + O2(g) ΔG° = -34.5 kJ

What can you conclude about ΔG°rxn for the reaction at 25°C? H2(g) + Br2(g) ⇌ 2 HBr(g) K = 2 × 1019

Calculate ?S°_rxn for the following reaction.The S° for each species is shown below the reaction. C₂H₂(g) + H₂(g) ? C₂H₄(g) S°(J/mol?K) 200.9 130.7 219.3

Determine the equilibrium constant for the following reaction at 298 K. Cl(g) + O₃(g) → ClO(g) + O₂(g) ΔG° = -34.5 kJ

What can you conclude about ΔG°_rxnfor the reaction at 25°C? H₂(g) + Br₂(g) ⇌ 2 HBr(g) K = 2 × 10¹⁹