1
Question
For the reaction at 300 K,
A(g)+B(g)→C(g)
△E=−3.0 k cal;△S=−10.0 cal/K, then the value of △G is:
For the reaction at 300 K,
A(g)+B(g)→C(g)
△E=−3.0 k cal;△S=−10.0 cal/K, then the value of △G is:
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Solution
The correct option is B −600 cal
Given, T=300 K, △E=−3.0 Kcal △S=−10 cal/K
A(g)+B(g)→C(g) R=2cal/K
△ng=1−1−1=−1
△G=△H−T△S
△H=△E+△ngRT
△G=△E+△ngRT−T△S
=−3000 cal+(−1×2×300)cal+(3000 cal)
△G=−600 cal
Given, T=300 K, △E=−3.0 Kcal △S=−10 cal/K
A(g)+B(g)→C(g) R=2cal/K
△ng=1−1−1=−1
△G=△H−T△S
△H=△E+△ngRT
△G=△E+△ngRT−T△S
=−3000 cal+(−1×2×300)cal+(3000 cal)
△G=−600 cal
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