For the given reaction: \(2A(g) + B(g) + C(s) \rightarrow 2D(g) \) \(\Delta \mathrm{U}^{\circ}=-10.5 \mathrm{~kJ} \text { and } \Delta \mathrm{S}^{\circ}=-44.1 \mathrm{JK}^{-1} \)
The value of \(\Delta G^o \) for the above reaction at 25 °C will be :
1.
1.2 kJ
2.
0.16 kJ
3.
3.2 kJ
4.
1.6 kJ
Subtopic: Gibbs Energy Change |
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