(a) A cell notation is shown below. Ni(s)/Ni2+(aq)// Sn4+(aq),Sn2+(aq)/Pt(s) (i) Identify the anode and cathode terminal by writing the equation for the reaction occurring in each half-cell, and hence write a balanced equation for the overall reaction which takes place when current flows. (ii) Calculate the Eo cell of this cell reaction. Given Eo Ni2+/Ni = +0.34 V, Eo Sn4+/Sn2+(aq)= +0.77 V
(a) A cell notation is shown below.
Ni(s)/Ni2+(aq)// Sn4+(aq),Sn2+(aq)/Pt(s)
(i) Identify the anode and cathode terminal by writing the equation for the
reaction occurring in each half-cell, and hence write a balanced equation
for the overall reaction which takes place when current flows.
(ii) Calculate the Eo cell of this cell reaction.
Given Eo Ni2+/Ni = +0.34 V,
Eo Sn4+/Sn2+(aq)= +0.77 V
(b) Cr3+ (aq) + 3e- → Cr(s) Eo = -0.74V
Br2(l) + 2e- → 2Br-(aq) Eo = +1.09V
(i) Based on the data above, construct a voltaic cell and label clearly on the
diagram: anode, cathode, the electrons movement and the electrolytes used
for both half-cells.
(ii) Write the equations for the reaction at anode and cathode
(iii) Write the overall cell reaction
(iv) Calculate the cell voltage (e.m.f.) of the cell
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