electrode reaction	$E^{⊖}$ / V
Cl $_{2}$ + 2e $^{-}$ $⇌$ 2Cl $^{-}$	+1.36
Cu $^{2 +}$ + 2e $^{-}$ $⇌$ Cu	+0.34
Fe(OH) $_{3}$ + e $^{-}$ $⇌$ Fe(OH) $_{2}$ + OH $^{-}$	$- 0.56$
Fe $^{3 +}$ + e $^{-}$ $⇌$ Fe $^{2 +}$	+0.77
V $^{2 +}$ + 2e $^{-}$ $⇌$ V	$- 1.13$
V $^{3 +}$ + e $^{-}$ $⇌$ V $^{2 +}$	$- 0.26$

Complete the equation that can be used to calculate the standard Gibbs free energy change,

Δ G^{⊖}

, for a cell reaction using the standard cell potential,

E_{ce l l}^{⊖}

4(b)Electrode Potentials Cell Free EnergyMedium2 marks

An electrochemical cell is set up using a V

^{3 +}

^{2 +}

electrode and a Cu

^{2 +}

/Cu electrode, both under standard conditions. Write an equation for the cell reaction that occurs and calculate the value for

E_{ce l l}^{⊖}

Equation

0 words

4(c)Electrode Potentials Cell Free EnergyMedium2 marks

Identify two atoms or ions from Table 4.1 that will reduce Fe

^{3 +}

to Fe

^{2 +}

under neutral conditions, but will not reduce Fe(OH)

_{3}

to Fe(OH)

_{2}

under alkaline conditions.

Two answers required.

4(d)Electrode Potentials Cell Free EnergyMedium2 marks

Identify the strongest oxidising agent and the strongest reducing agent in Table 4.1.

strongest oxidising agent

strongest reducing agent

4(e)ElectrolysisHard3 marks

A dilute solution of NaOH(aq) is electrolysed using inert electrodes. A steady current of 2.40 A is passed for 2.00 hours. Calculate the mass, in g, of oxygen that is released at the anode.

mass of oxygen

0 words