NEET2026ChemistryChapterActual
Consider the following electrochemical cell reaction: Cr ( s ) + 3 Ag ⁺( aq ) Cr ³⁺( aq ) + 3 Ag ( s ) If the standard cell potential ( E^ _ cell ) is 1.54 V , determine the standard Gibbs free energy change ( G^ ) for the process. (Given: 1 F = 96487 C mol ⁻¹ )
Options
- A-148.59 kJ mol ⁻¹
- B-445.77 J mol ⁻¹
- C-445.77 kJ mol ⁻¹
- D+445.77 kJ mol ⁻¹
Correct answer
C. -445.77 kJ mol ⁻¹
Step-by-step solution
The standard Gibbs free energy change is given by the relation: G^ = -nFE^ _ cell For the given reaction, the number of electrons transferred is n = 3 . Substituting the given values: G^ = -3 96487 C mol ⁻¹ 1.54 V G^ = -445769.94 J mol ⁻¹ G^ -445.77 kJ mol ⁻¹ Answer: -445.77 kJ mol ⁻¹