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

[H⁺] = 1.30X10⁻⁴ M

Step-by-step explanation:

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

`E_(cell)=E^(0)_(cell)- (0.0592)/(n)logQ`

In the given equation

n = 2

Q =
`=([Zn^(+2)][p_(H2)])/([H^(+)]^(2))`

Putting values

`0.53= 0.76 - (0.0592)/(n)log((1X1)/([H^(+)]^(2)))`

on calculating

[H⁺] = 1.30X10⁻⁴ M