The `EMF` of the following cell is observed to be `0.118V` at `25^(@)C:`

If `30mL` of `0.2M NaOH` is added to the negative terminal of the battery, find the `EMF` of the cell.

The emf of the following cell is observed to be 0.118V at 25^(@)C . [Pt,H_(2)(1atm)|HA(100mL 0.1M||H^(o+)(0.1M)|H_(2)(1atm)|Pt] a. If 30mL of 0.2M NaOH is added to the negative terminal of battery, find the emf of the cell. b. If 50mL of 0.2 M NaOH is added to the negative terminal of battery, find the emf of teh cell.

The emf of the following cell is observed to be 0.118V at 25^(@)C . [Pt,H_(2)(1atm)|HA(100mL 0.1M||H^(o+)(0.1M)|H_(2)(1atm)|Pt] a. If 30mL of 0.2M NaOH is added to the negative terminal of battery, find the emf of the cell. b. If 50mL of 0.2 M NaOH is added to the negative terminal of battery, find the emf of teh cell.

Define - terminal voltage of the cell? What is the e.m.f of a cell?

Four cells, each of e.m.f 1.5 V, are connected in series to form a battery. Find the e.m.f of the bettery.

If the e.m.f of a galvanic cell is negative, it implies that:

If the e.m.f of a galvanic cell is negative , it implies that :

The standard EMF of a galvanic cell involving cell reaction with n=2 is found to be 0.295 V at 25^(@)C . The equilibrium constant of the reaction would be

The standard emf of a galvanic cell involving cell reaction with n = 2 is formed to be . 0.295 V at 25^(@)C . The equilibrium constant of the reaction would be :