JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
The value of \(\log\,K\) for the reaction \(A \leftrightharpoons B\) at \(298\,K\) is (Nearest integer) Given: \(\Delta H ^0=-54.07\,kJ\,mol ^{-1}\) \(\Delta S ^{\circ}=10\,JK ^{-1}\,mol ^{-1}\) (Take \(2.303 \times 8.314 \times 298=5705\) )
- A \(11\)
- B \(12\)
- C \(14\)
- D \(10\)
Answer & Solution
Correct Answer
(D) \(10\)
Step-by-step Solution
Detailed explanation
\(\Delta G ^0=\Delta H ^0- T \Delta S\) \(\Rightarrow \Delta G ^0=(-54070-10 \times 298)\) Also, \(\Delta G ^0=(-2.303 RT \log K )\) \(\Rightarrow(-54070-10 \times 298)\) \(=(-2.303 \times 8.134 \times 298 \log K )\) \(\Rightarrow \log K =10 \text { Ans: } 10\)
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