Given the information A+BC⟶2D⟶DΔ𝐻∘Δ𝐻∘=662.4 kJΔ𝑆∘=298.0 J/K=539.0 kJΔ𝑆∘=−172.0 J/K calculate Δ𝐺∘ at 298 K for the reaction A+B⟶2C Δ𝐺∘=

Answer 1

Given the information A+BC⟶2D

Δ𝐻∘=662.4 kJ, Δ𝑆∘=298.0 J/K

C⟶D Δ𝐻∘=539.0 kJ, Δ𝑆∘=−172.0 J/K

calculate Δ𝐺∘ at 298 K for the reaction A+B⟶2C

Answer: To calculate the standard Gibbs free energy change for the reaction A+B⟶2C, we can use the equation:

Δ𝐺∘ = Δ𝐻∘ - TΔ𝑆∘

where Δ𝐻∘ is the standard enthalpy change, Δ𝑆∘ is the standard entropy change, and T is the temperature in Kelvin.

We can start by finding the standard Gibbs free energy change for the formation of 2D from A and BC, using the given equation and values:

Δ𝐺∘ = Δ𝐻∘ - TΔ𝑆∘ Δ𝐺∘ = 662.4 kJ - (298 K * 0.2980 kJ/K) Δ𝐺∘ = 571.3 kJ

Next, we can find the standard Gibbs free energy change for the conversion of C to D, using the given equation and values:

Δ𝐺∘ = Δ𝐻∘ - TΔ𝑆∘ Δ𝐺∘ = 539.0 kJ - (298 K * (-0.1720 kJ/K)) Δ𝐺∘ = 590.1 kJ

Now we can use the given reaction A+BC⟶2D and the known standard Gibbs free energy changes to find the standard Gibbs free energy change for the reaction A+B⟶2C:

A+BC⟶2D

2C⟶2D + B

We can reverse the second equation, multiply it by 2 to match the coefficients of the first equation, and add the two equations together:

2C⟶2D + B (reverse and multiply by 2) Δ𝐺∘ = -2(590.1 kJ) = -1180.2 kJ

A+BC⟶2D Δ𝐺∘ = 571.3 kJ

A+B⟶2C Δ𝐺∘ = -1180.2 kJ - 571.3 kJ Δ𝐺∘ = -1751.5 kJ

Therefore, the standard Gibbs free energy change for the reaction A+B⟶2C at 298 K is -1751.5 kJ.