The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is (F = 96,500 C mol–1, R = 8.314 JK–1 mol–1)(a) 1.0 × 101 (b) 1.0 × 1030 (c) 1.0 × 1010 (d) 1.0 × 105

The standard emf of a cell involving one electron change is found to b

1.	The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is (F = 96,500 C mol–1, R = 8.314 JK–1 mol–1)(a) 1.0 × 101 (b) 1.0 × 1030 (c) 1.0 × 1010 (d) 1.0 × 105
Answer» Hola User__________________ Here is Your Answer..!!! _________________________ ⭐Actually welcome to the concept of the ELECTROCHEMISTRY ⭐Basically APPLYING the GIBBS ENERGY equation for the Equilibrium condition of the EMF of the cell we get as ⭐E° = 0.0591/n . log (k~eq) ⭐since here the CHANGE in e~ is 1 and the E° = 0.591 ⭐we get the answer as ⭐K~eq = 1 × 10^10 ____________________________ HOPE It helps u....☺