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JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry

Consider the reaction \(X \rightleftharpoons Y\) at \(300\) K. If \(\Delta H^{\theta}\) and \(K\) are \(28.40\) kJ mol\(^{-1}\) and \(1.8 \times 10^{-7}\) at the same temperature, then the magnitude of \(\Delta S^{\theta}\) for the reaction in J K\(^{-1}\) mol\(^{-1}\) is _______. (Nearest integer) (Given: \(R = 8.3\) J K\(^{-1}\) mol\(^{-1}\), \(\ln 10 = 2.3\), \(\log 3 = 0.48\), \(\log 2 = 0.30\))

  1. A 30
  2. B 32
  3. C 34
  4. D 36
Verified Solution

Answer & Solution

Correct Answer

(C) 34

Step-by-step Solution

Detailed explanation

The standard Gibbs free energy change is given by: \(\Delta G^{\theta} = -RT \ln K = -2.3 RT \log K\) First, calculate \(\log K\): \(\log K = \log(1.8 \times 10^{-7}) = \log(18 \times 10^{-8})\) \(\log K = \log 18 - 8 = \log(2 \times 3^2) - 8\) \(\log K = \log 2 + 2 \log 3 - 8\)…
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