Electrochemistry Mock Tests

For the cell Zn | Zn²⁺(0.01 M) || Cu²⁺(1.0 M) | Cu at 298 K, if E°cell = 1.10 V, the cell potential is:

What is the standard electrode potential (E°) of a cell if ΔG° for the cell reaction is negative?

The standard electrode potential for the cell Zn|Zn²⁺||Cu²⁺|Cu is (E°(Zn²⁺/Zn) = -0.76 V, E°(Cu²⁺/Cu) = +0.34 V):

A current of 2.0 A is passed through an aqueous solution of CuSO₄ for 965 seconds. The mass of copper deposited at the cathode is (Atomic mass of Cu = 63.5, F = 96500 C/mol):

The cell potential of a Daniell cell (E° = 1.1 V) becomes zero when:

The same quantity of electricity that deposits 1.08 g of silver from AgNO₃ solution will deposit how much copper from CuSO₄ solution? (Atomic masses: Ag = 108, Cu = 63.5)

Three electrolytic cells containing aqueous solutions of AgNO₃, CuSO₄, and AuCl₃ are connected in series. If the same current is passed through all three cells, what is the ratio of moles of metal deposited at the cathode (Ag : Cu : Au)?

The standard electrode potentials are: E0(Zn2+/Zn) = -0.76 V and E0(Cu2+/Cu) = +0.34 V. What is the standard EMF of the cell: Zn | Zn2+(1M) || Cu2+(1M) | Cu?