How much time is required for complete decomposition of 4 mol of water using a current of 4 ampere?

Question

How much time is required for complete decomposition of 4 mol of water using a current of 4 ampere? (A) 1.93× 105 sec (B) 3.85× 104 sec (C) 96500 sec (D) 2.92× 105 sec

Tardigrade Admin · Accepted Answer

To decompose 1 mole of H 2 O, we need two moles of electrons. To decompose 4 moles of H 2 O, we need 8 Faraday. Now, Q=I × t ⇒ t =(8 × 96500/4) =1.93 × 105 sec

Q. How much time is required for complete decomposition of $4 m o l$ of water using a current of $4$ ampere?

$1.93 \times 1 0^{5} sec$

$3.85 \times 1 0^{4} sec$

$96500 sec$

$2.92 \times 1 0^{5} sec$

To decompose $1$ mole of $H_{2} O$ , we need two moles of electrons.
To decompose $4$ moles of $H_{2} O$ , we need $8$ Faraday.
Now, $Q = I \times t$
$\Rightarrow t = \frac{8 \times 96500}{4}$
$= 1.93 \times 1 0^{5} sec$

Q. How much time is required for complete decomposition of 4mol of water using a current of 4 ampere?

1.93×105sec

3.85×104sec

96500sec

2.92×105sec