For this reaction at 300 K A g - B g - C g - U -3-0 kcal - - S -10-0 cal - K value of G is -A- 600 calB- 6600 calC- -600 calD- -6600 cal

The correct option is C 600 calGiven, nbsp;A(g) + B(g) → C(g)U = 3.0 kcal; nbsp; S = 10.0 cal/K for above reaction Δ n_g= 1 We know the relationG = ...

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

For this reac...

Question

For this reaction at 300 K $A (g) + B (g) \to C (g) △ U = - 3.0 k c a l; △ S = - 10.0 c a l / K$ value of $△ G$ is :

- 600 c a l

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- 6600 c a l

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600 c a l

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6600 c a l

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Solution

The correct option is A $- 600 c a l$
Given, $A (g) + B (g) \to C (g)$ $△ U = - 3.0 k c a l; △ S = - 10.0 c a l / K$
for above reaction $Δ n_{g} = - 1$
We know the relation $△ G = △ H - T △ S$
Also, $△ H = △ U + △ n_{g} R T$
$= - 3000 - 1 \times 2 \times 300$
( Putting R = 2 cal ) \)
$△ H = - 3600 c a l$
$∴ △ G = - 3600 + 300 \times 10 = - 600 C a l$

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For this reaction at 300 K A(g)+B(g)→C(g) △U=−3.0 kcal;△S=−10.0 cal/K value of △G is :

The correct option is A −600 calGiven, A(g)+B(g)→C(g) △U=−3.0 kcal;△S=−10.0 cal/K for above reaction Δng=−1 We know the relation△G=△H−T△S Also, △H=△U+△ngRT =−3000−1×2×300 ( Putting R = 2 cal ) \) △H=−3600 cal ∴△G=−3600+300×10=−600 Cal

For this reaction at 300 K $A (g) + B (g) \to C (g) △ U = - 3.0 k c a l; △ S = - 10.0 c a l / K$ value of $△ G$ is :