JEE Advanced2012ChemistryElectrochemistryActual
The electrochemical cell shown below is a concentration cell. M M ²⁺ (saturated solution of a sparingly soluble salt, . MX ₂ ) | M ^ 2 (0.001 ~mol dm ⁻³ ) M . The emf of the cell depends on the difference in concentrations of M ²⁺ ions at the two electrodes. The emf of the cell at 298 ~K is 0.059 ~V . Question: The value of G ( kJ mol ⁻¹ ) for the given cell is (take 1 F =96500 Cmol ⁻¹ )
Options
- A-5.7
- B5.7
- C11.4
- D-11.4
Correct answer
D. -11.4
Step-by-step solution
At anode : M( ~s )+2 X⁻( aq ) M X₂( aq )+2 e ⁻ At cathode : M⁺²( aq )+2 e ⁻ M( ~s ) Thus, here n=2 G=-n F E_ cell =-2 96500 0.059 10⁻³ ~kJ / mole =-11.4 ~kJ / mole