Question

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.53 V. The concentration of H+ in the cathode compartment is ________ M.

Answer 1

Answer:

[H⁺] = 1.30X10⁻⁴ M

Explanation:

the problem will be solved by using Nernst's equation, which is :

$E_{cell}=E^{0}_{cell}- \frac{0.0592}{n}logQ$

In the given equation

n = 2

Q = $=\frac{[Zn^{+2}][p_{H2}]}{[H^{+}]^{2}}$

Putting values

$0.53= 0.76 - \frac{0.0592}{n}log(\frac{1X1}{[H^{+}]^{2}})$

on calculating

[H⁺] = 1.30X10⁻⁴ M