Kuiz Electrochemistry (Nernst, Faraday)

Faraday's first law stated that

(a)  

Faraday's second law stated that

(a)  

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

• +0.28V

• +0.31V

• +0.35V

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 = ??

• +0.14 V

• +0.16 V

• +0.20V

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

• +0.26 V

• +0.28 V

• +0.30V

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.

• 21.69 g

• 22.69 g

• 23.69 g

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.

• 0.27 g

• 0.29 g

• 0.40 g

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]

• 1567 cm³

• 1580 cm³

• 1667 cm³

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

• 1.58 X 10⁴ s

• 1.68 X 10⁴ s

• 1.78 X 10⁴ s

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)

• +0.41 V

• +0.51 V

• +0.61 V