The EMF of a cell corresponding to the reaction- Zns - 2H-aq - Zn2-0-1 M - H2g- 1 atm is 0-82 V at 25-C-The pH of the solution at the hydrogen electrode is- E-Zn2- - Zn - - 0-76 V E-H- - H2 - 0If the value is 63-10-x- then what is the value of x-

Half cell reactions are : [Zn(s) → Zn^2+(aq) + 2e^ ] at anode [H^⊕ + e^ → 1/2 H_2] at cathodeFor zinc electrode: E_Zn | Zn^2+ = E^⊝_Zn ...

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Nernst Equation

The EMF of a ...

Question

The EMF of a cell corresponding to the reaction:
$Z n (s) + 2 H^{⨁} (a q) \to Z n^{2 +} (0.1 M) + H_{2} (g, 1 a t m)$ is $0.82 V$ at $25^{\circ} C$ .
The pH of the solution at the hydrogen electrode is:
$E_{Z n^{2 +} | Z n}^{⊝} = - 0.76 V$
$E_{H^{⊝} | H_{2}}^{⊝} = 0$
If the value is $63 \times 10 - x$ , then what is the value of x?

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