9. Calculate ΔG0 at 820C for reactions in which (a) ΔH0= 293 kJ; ΔS0 = -695...

Question

Question

9. Calculate ΔG0 at 820C for reactions in which

(a) ΔH0= 293 kJ; ΔS0 = -695 J/K

(b) ΔH0= -1137 kJ; ΔS0= 0.496 kJ/K

Answer 1

Answer #1

G⁰ = H⁰ -TS⁰

We use this formula for both the below questions

T = 82⁰C = (82+273)K = 355K

(a) H⁰ = 293kJ = 293000J [Since 1kJ = 1000J]

G⁰ = H⁰ -TS⁰

G⁰ = 293000J - (355K x -695J/K)

G⁰ = 293000J + 246725J = 539725J

(b) H⁰ = -1137kJ

G⁰ = H⁰ -TS⁰

G⁰ = -1137kJ - (355K x 0.496kJ/K)

G⁰ = -1137kJ - 176.08kJ

G⁰ = 1313.08kJ = 131080J

Answer 2

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