Question

How many grams of nickel metal are plated out when a constant current of 15.0

A is passed through aqueous NiCl2 for 60.0 minutes?
A) 10.9 gB) 16.4 gC) 32.8 gD) 36.3 g

Answer 1

Answer:

B) 16.4

Explanation:

Given that:-

Current, I = 15.0 A

Time, t = 60.0 minutes

Also, 1 minute = 60 seconds

So, t = $60\times 60$ s = 3600 s

F is Faraday constant = 96485 C

Atomic weight of Nickel = 58.69 g/mol

Also, Charge on Ni in $NiCl_2$ = 2

So, equivalent weight of Ni , E = $\frac{58.69}{2}\ g/mol$ = 29.34 g/mol

Thus, according to the Faraday's Law:-

$W=\frac{EIt}{96485}$

Where, W is the mass of the metal deposited.

So,

$W=\frac{29.34\times 15\times 3600}{96485}\ g=16.4\ g$

Weight of Ni metal plated out = 16.4 g