Calculate the E of following half cell.
Cu2+(aq) (0.1 M) + 2e-  $\rightarrow$  Cu(s)

Calculate the standard electrode potential for the following half cell.
Sn4+ (aq)(1.0 M) + 2e-  $\rightarrow$  Sn2+(aq) (1.0 M) E0 = +0.15 V

Sn4+ (aq)(0.2 M) + 2e- $\rightarrow$   Sn2+(aq) (0.4 M) E = ??

Calculate the e.m.f of the electrochemical cell.

A current of 5.0 A flows for 4 hours through an aqueous solution of copper sulphate (VI). Calculate the mass of copper deposited at the cathode.

When a certain amount of electric charge flows through an aqueous solution of silver nitrate, 3.24 g of silver is deposited on the cathode.

Calculate the mass of aluminium, Al that will be deposited by the same quantity of charge.

An aqueous solution of chromium(III) sulphate was electrolysed for five hours, using a constant current of 1.5 A. Calculate the volume of oxygen gas produced at s.t.p. [Ar Cr:52.0; F=96 500 C mol^-1]

Calculate the time taken to produce 18.0 g of silver from silver nitrate by a current of 0.900 A.

Calculate the e.m.f. of the electrochemical cell.

Cr(s) l Cr³⁺(aq, 0.010 M) ll Ni²⁺ (aq, 0.20 M) l Ni (s)