Calculate E^0_ cell for following Zn_ (s) ,| ,Zn^ ++ _ (1M) ,|| ,Pb^ ++ _ (1M) ,| ,Pb_ (s) if E^0_ Zn = -0.763 , V and E^0_ Pb = -0.126 , V

MHT CET 2023 Chemistry question

Calculate for following \mathrm{Zn_{(s)}\,|\,Zn^{++}_{(1M)}\,||\,Pb^{++}_{(1M)}\,|\,Pb_{(s)}} if and

(A)0.637 VCorrect
(B)-0.530 V
(C)-0.889 V
(D)0.789 V

Answer: (A)

Solution

In the cell notation the left electrode (Zn) is the anode (oxidation) and the right electrode (Pb) is the cathode (reduction). E^0_{cell} = E^0_{cathode} - E^0_{anode} = E^0_{Pb^{2+}/Pb} - E^0_{Zn^{2+}/Zn} = (-0.126) - (-0.763) = +0.637\ V: option (a).

See the full step-by-step solution

Create a free account to read the complete working, and practise questions like this in a timed test.

Create a free account

Question ID VK-097875