15. NEED HELP FAST

Question

Given the information

A+B⟶2D Δ𝐻∘ =-677.5kJ Δ𝑆∘= 370.0 J/K

C⟶D Δ𝐻∘ = 509.0kJ Δ𝑆∘=-243.0 J/K

calculate  Δ𝐺∘  at 298 K for the reaction

A+B⟶2C

Δ𝐺∘=

Answer 1

A+B⟶2D Δ𝐻∘ =-677.5kJ Δ𝑆∘= 370.0 J/K

C⟶D Δ𝐻∘ = 509.0kJ Δ𝑆∘=-243.0 J/K

calculate  Δ𝐺∘  at 298 K for the reaction

A+B⟶2C

For this problem, we want to use Hess' Law. (Please do check my math)

Copy eq. 1: A + B ==> 2D ... ∆H = -677.5 kJ; ∆S = 370 J/K = 0.370 kJ/K

Reverse eq. 2 and multiply by 2: 2D ==> 2C ... ∆H = 2 x -509 kJ = 1018 kJ; ∆S = 2 x 243 J/K = 0.486 kJ/K

Add the 2 equations:

A + B + 2D ==> 2D + 2C which reduces to A + B ==> 2C

∆H = -677.5 kJ + (-1019) = -1697 kJ

∆S = 0.370 kJ/K + 0.486 kJ/K = 0.856 kJ/K

∆G = ∆H - T∆S = -1697kJ - (298K)(0.856 kJ/K)

∆G = -1697 kJ - (298)(0.856)

∆G = -1952 kJ

Answer 2

The answer would be -1949 kJ. Lmk if you need an explanation