Electrochemical Cells (DP IB Chemistry: HL)

Use the following electrode potentials to answer the question.

Sn²⁺ (aq) + 2e^- ⇌ Sn (s)      E^θ = -0.14 V

Fe³⁺ (aq) + e^- ⇌  Fe²⁺ (aq)  E^θ = +0.77 V

What will be the EMF, in V, when the following voltaic cell is connected?

Sn (s) + 2Fe³⁺ (aq) → 2Fe²⁺ (aq) + Sn²⁺ (aq)

Which of the following reactions could take place at the positive electrode (cathode) in a voltaic cell? 

1.   Cu²⁺ (aq) to Cu (s)
2.   Br₂ (g) to Br^- (aq)
3.   Co³⁺ (aq) to Co²⁺(aq)

What is true when aqueous copper(II) sulfate is electrolysed using platinum electrodes?

Use the following electrode potentials to answer the question. 

Zn²⁺ (aq) + 2e^- ⇌ Zn (s)      E^θ = -0.76 V

Cl₂ (aq) + 2e^- ⇌  2Cl^- (aq)   E^θ = +1.36 V

Mg²⁺ (aq) + 2e^- ⇌ Mg (s)     E^θ = -2.37 V 

Predict what happens when some powdered zinc is added to aqueous magnesium chloride?

Which of the following electrolytic cells would give the greatest mass of metal at the cathode?

Which of the following can be used for a standard hydrogen electrode (SHE)?

What are the ratios of gases produced at the electrodes in the electrolysis of dilute vs concentrated sodium chloride solution?

Which of the following could be used to electroplate a zinc medal?

The diagram below shows the set-up of aluminium and silver cells in series:

What calculation shows the loss in mass of the aluminium electrode if the silver electrode gains 0.25 g?

The oxidation of iron is a spontaneous process described by the overall equation:

Fe (s) + O₂ (g) + H₂O (l) → Fe(OH)₂ (s)       

(ΔG^θ = -164 kJ mol^-1 at 298 K)

The two half equations for the process are:

Fe²⁺ (s) + 2e^- → Fe (s)

O₂ (g) + H₂O (l) + 2e^- → 2OH^- (s)

(ΔG^θ = -nFE^θ , F = 9.65 x 10⁴  C mol^-1)

Which is the correct calculation to work out E^θ in V?