1
Question
For the reaction at 300K
A(g)+B(g)→C(g);ΔE=−3.0 kcal; ΔS=−10.0 cal/K value of ΔG is:
For the reaction at 300K
A(g)+B(g)→C(g);ΔE=−3.0 kcal; ΔS=−10.0 cal/K value of ΔG is:
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Solution
The correct option is D None
For the reaction A(g)+B(g)→C(g)T=300K;ΔE=ΔU−3.0 kcal; ΔS=−10.0 cal/K ΔG=ΔH−TΔSΔH=ΔU+ΔngRTΔH=−3000+(1−2)×1.987×300ΔH=−3594 calthus ΔG=−3594−300×(−10)ΔG=−594 cal
For the reaction
A(g)+B(g)→C(g)
T=300K;ΔE=ΔU−3.0 kcal; ΔS=−10.0 cal/K
ΔG=ΔH−TΔS
ΔH=ΔU+ΔngRT
ΔH=−3000+(1−2)×1.987×300
ΔH=−3594 cal
thus ΔG=−3594−300×(−10)
ΔG=−594 cal
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