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Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq)...

Consider the voltaic cell and reduction half potentials:

Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq) (1.50 M) | Ni(s)

Zn 2+ (aq)/Zn (s) E o = - 0.760 V

Ni2+ (aq)/Ni (s) E o = - 0.230 V

a) Sketch the voltaic cell represented with the above line notation. Label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution. Also indicate the direction of electron flow (3 marks).

b) What is Ecell initially? (2 marks). c) What will be Ecell when [Ni2+] has fallen to 0.500 M? (2 marks).

c) What are the ion concentrations of Ni2+ and Zn2+ when Ecell falls to 0.450

d) What are the ion concentrations of Ni2+ and Zn2+ when Ecell falls to 0.450 V? (3 marks).

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