AP EAMCET · Chemistry · Thermodynamics (C)
At the temperature \(T(\mathrm{~K})\) for the reaction \(X_2 \mathrm{O}_4(l) \rightarrow 2 X \mathrm{O}_2(g) \Delta U=x \mathrm{~kJ} \mathrm{~mol}^{-1}\), \(\Delta S=y \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\). Gibbs energy change for the reaction is (Assume \(X_2 \mathrm{O}_4, X_2\) are ideal gases) \(\Delta U=x \mathrm{~kJ} \mathrm{~mol}^{-1}, \Delta S=y \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\)
- A \(1000 x+2 R(T-y) \mathrm{J} \mathrm{mol}^{-1}\)
- B \(1000 x+T(2 R-y) \mathrm{J} \mathrm{mol}^{-1}\)
- C \(x+T(2 R-y) \mathrm{J} \mathrm{mol}^{-1}\)
- D \(x+2 R(T-y) \mathrm{J} \mathrm{mol}^{-1}\)
Answer & Solution
Correct Answer
(B) \(1000 x+T(2 R-y) \mathrm{J} \mathrm{mol}^{-1}\)
Step-by-step Solution
Detailed explanation
But, \(\quad H=U+p V\) or \(H=U+n R T\) From equation (i) and (ii) we get \[ \Delta G=\Delta U+\Delta n R T-T \Delta S \] But, for given reaction. \(\Delta n=2, \Delta U=1000 \times \mathrm{J} / \mathrm{mol}\) and \[ \Delta S=y \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \]…
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