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Question

For the reaction at 300 K


A(g)+B(g)C(g)

ΔH=3.0 kcal;ΔS=10.0cal/K value of ΔG is:

A
600cal
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B
6600cal
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C
6000cal
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D
none
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Solution

The correct option is C 6600cal
A(g)+B(g)C(g)

The change in Gibb's free energy is given by

ΔG=ΔHTΔS

whereas,

ΔH= Enthalpy of reaction

ΔS= Entropy of reaction =10cal/K

As we know that,

ΔH=ΔU+ΔngRT

whereas,

ΔU= Change in internal energy =3kcal=3000cal

Δng=nPnR=1(1+1)=1

R= Gas constant =2cal

T=300K

ΔH=3000+(1×2×300)=3600cal

ΔG=3600(300×(10))=36003000=6000cal

Hence the value of ΔG is 6600cal.

Hence, the correct option is B

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