333
Question
For the reaction at 300K
A(g)+B(g)⟶C(g)
ΔU=−3.0kcal;ΔS=−10.0cal/K
Value of ΔG is:
For the reaction at 300K
A(g)+B(g)⟶C(g)
ΔU=−3.0kcal;ΔS=−10.0cal/K
Value of ΔG is:
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Solution
The correct option is A −600cal
ΔG=ΔH−TΔSΔG=ΔU+RTΔn−TΔS
T=300 K,Δn=−1ΔU=−3000 cal,ΔS=−10 calΔG=−3000+(−2×300)−(−10)(300)ΔG=−600 calOption A is correct.
ΔG=ΔH−TΔS
ΔG=ΔU+RTΔn−TΔS
T=300 K,Δn=−1
ΔU=−3000 cal,ΔS=−10 cal
ΔG=−3000+(−2×300)−(−10)(300)
ΔG=−600 cal
Option A is correct.
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