JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
For the reaction taking place in the cell: \(Pt ( s )\left| H _{2}( g )\right| H ^{+}( aq ) \| Ag ^{+}( aq ) \mid Ag ( s )\) \(E _{\text {Cell }}^{0}=+0.5332 V\). The value of \(\Delta_{ f } G ^{0}\) is \(kJ \,mol ^{-1} \cdot\) (in nearest integer)
- A \(5\)
- B \(96\)
- C \(51\)
- D \(57\)
Answer & Solution
Correct Answer
(C) \(51\)
Step-by-step Solution
Detailed explanation
\(\frac{1}{2} H _{2}+ Ag ^{+} \rightarrow H ^{+}+ Ag\) \(\Delta G ^{\circ}=- nE ^{\circ} F\) \(=-1 \times 0.5332 \times 96500 \,J\) \(=-51.35 \,kJ\) \(\left( n =2 \text { for } H _{2}+2 Ag ^{+} \rightarrow 2 H ^{+}+2 Ag \right)\)
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