calculate for ΔG

Question

For a particular reaction at  219.6°C, Δ𝐺=−139.48 kJ/mol  and Δ𝑆=594.04 J/(mol⋅K)

Calculate ΔG for this reaction at  -11.4°C.

Answer 1

∆G = ∆H - T∆S

∆G = -139.48 kJ/mol

∆H = ?

T = 219.6C + 273.15 = 492.8K

∆S = 594.04 J/molK = 0.59404 kJ/molK

Solving for ∆H we have ∆H = ∆G - T∆S

∆H = -139.48 kJ/mol - (492.8K)(0.59404 kJ/molK)

∆H = -139.48 kJ/mol - 292.74 kJ/mol)

∆H = -432.22 kJ/mol

Using this value of ∆H, find ∆G at -11.4ºC = 261.8K

∆G = ∆H - T∆S

∆G = -432.22 - (261.8)(0.59404)

∆G = -432.22 - 155.49

∆G = -587.71 kJ/mol