A galvanic cell is set up from a zinc bar weighing `100g` and `1.0L` of `1.0M CuSO_(4)` solution. How long would the cell run if it is assumed to deliver a steady current of `1.0A. (` Atomic mass of `Zn=65)`.

Options

A. `1.1` hours
B. 46 hours
C. `53.6` hourse
D. 24 hours.

Answer

c

Explanation

Mole of `Zn=(100)/(65.3)=1.53mol`
Mole of `Cu^(2+)=1xx1=1 mol `
So `Zn` is in excess, hence `Cu^(2+)` will react completely.
`Cu^(2+)+2e^(-) rarr Cu`
`2F-=1 mol `of `Cu`
`2xx96500C-=1.0Axxt(` in seconds `)`
`t=(2xx96500)/(3600)h=53.6h`