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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.

Respuesta :

Answer:

[H⁺] = 1.30X10⁻⁴ M

Explanation:

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

[tex]E_{cell}=E^{0}_{cell}- \frac{0.0592}{n}logQ[/tex]

In the given equation

n = 2

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

Putting values

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

on calculating

[H⁺] = 1.30X10⁻⁴ M

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