NEET2026ChemistryChapterActual
For the galvanic cell reaction given below: 2 Cr(s) + 3 Cd ²⁺ (aq) 2 Cr ³⁺ (aq) + 3 Cd(s) The standard cell potential ( E^ _ cell ) is 0.34 V . Calculate the standard Gibbs free energy change ( G^ ) for the reaction. (Given: 1 F = 96500 C mol ⁻¹ )
Options
- A-98.43 kJ mol ⁻¹
- B+196.86 kJ mol ⁻¹
- C-196.86 kJ mol ⁻¹
- D-65.62 kJ mol ⁻¹
Correct answer
C. -196.86 kJ mol ⁻¹
Step-by-step solution
The given cell reaction is: 2 Cr(s) + 3 Cd ²⁺ (aq) 2 Cr ³⁺ (aq) + 3 Cd(s) The number of electrons transferred in the balanced reaction is n = 6 . The standard Gibbs free energy change is given by the relation: G^ = -nFE^ _ cell Substituting the given values: G^ = -6 96500 0.34 G^ = -196860 J mol ⁻¹ G^ = -196.86 kJ mol ⁻¹ Answer: -196.86 kJ mol ⁻¹