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. 82.47 hrs
B. 53.61 hrs
C. 41.23 hrs
D. 26.80 hrs

Answer

B

Explanation

1L of 1.0 M `CuSO_(4)` solution contains `Cu^(2+)=1` mole
`100" g Zn"=(100)/(65)` mole
thus, in the cell reaction `Zn+Cu^(2+)toZn^(2+)+Cu,Cu^(2+)` ions are the limiting reagent. The cell will run till all the `Cu^(2+)` ions are deposited, i.e., 1 mole of Cu is deposited. quantity of electricity requried for deposition of 1 mole of Cu=2F
Time, `t=(2xx96500C)/(1A)=2xx96500s`
`=(2xx96500)/(3600)hr=53.61hr`