Open Question
What is δg° for the following reaction at 25 °C? COBr2(g) ⇌ CO(g) + Br2(g) Kp = 4.11 × 104
19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium
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At 1120 K, ΔG° = 78.9 kJ/mol for the reaction 3 A (g) + B (g) → 2 C (g). If the partial pressures of A, B, and C are 11.5 atm, 8.60 atm, and 0.510 atm respectively, what is the Gibbs free energy change (ΔG) for this reaction under these conditions?
A
ΔG = 72.6 kJ/mol
B
ΔG = 78.9 kJ/mol
C
ΔG = 90.3 kJ/mol
D
ΔG = 85.2 kJ/mol
Verified step by step guidance1
Identify the given values: ΔG° = 78.9 kJ/mol, partial pressures of A = 11.5 atm, B = 8.60 atm, and C = 0.510 atm.
Recall the formula for calculating the Gibbs free energy change under non-standard conditions: ΔG = ΔG° + RT ln(Q), where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.
Calculate the reaction quotient Q using the expression Q = (P_C^2) / (P_A^3 * P_B), where P_C, P_A, and P_B are the partial pressures of C, A, and B respectively.
Convert the temperature from Kelvin to the appropriate units for the gas constant if necessary, and substitute the values into the equation ΔG = ΔG° + RT ln(Q).
Solve for ΔG by calculating the natural logarithm of Q, multiplying by RT, and adding the result to ΔG°.
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