WBJEE · Chemistry · Thermodynamics (C)
The standard Gibbs free energy change \(\left(\Delta G^{o}\right)\) at \(25^{\circ} \mathrm{C}\) for the dissociation of \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{g})\) to \(\mathrm{NO}_{2}(g)\) is (given, equilibrium constant \(=0.15, R=8.314 \mathrm{JK} / \mathrm{mol})\)
- A \(1.1 \mathrm{KJ}\)
- B \(4.7 \mathrm{KJ}\)
- C \(8.1 \mathrm{KJ}\)
- D \(38.2 \mathrm{KJ}\)
Answer & Solution
Correct Answer
(B) \(4.7 \mathrm{KJ}\)
Step-by-step Solution
Detailed explanation
\[ \begin{array}{l} =-2.303 \times 8.314 \times 298 \times \log 0.15 \\ =-2.303 \times 8.314 \times 298 \times(-0.82) \\ =4678.7 \mathrm{J}=4.67 \mathrm{kJ} \end{array} \]
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