For a particular reaction at 128.1 °C, ΔG = 377.52 kJ/mol, and ΔS = 556.72 J/(mol·K).
Calculate ΔG for this reaction at -78.3 °C.
= ? kJ / mol
ΔG = ΔH -TΔS
T = 128.1 C0 = 128.1+273 = 401.1K
ΔG = 377.52 kJ/mol,
ΔS = 556.72 J/(mol·K) = 0.55672Kj/mole-K
ΔG = ΔH -TΔS
377.52 = ΔH -401.1*0.556.72
ΔH = 377.52+401.1*0.556.72 = 600.82KJ
T = -78.3 °C. = -78.3+273 = 194.7K
ΔG = ΔH -TΔS
= 600.82-194.7*0.55672 =492.43Kj/mole
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