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How many grams of nickel metal are plated out when a constant current of [tex]15.0 \, A[/tex] is passed through aqueous [tex]\text{NiCl}_2[/tex] for 60.0 minutes?

A) 10.9 g
B) 16.4 g
C) 32.8 g
D) 36.3 g

Answer :

Final answer:

To determine the mass of nickel metal plated out, use Faraday's law of electrolysis and the given values of current and time. The answer is 16.4 grams.

Explanation:

To determine the number of grams of nickel metal plated out, we need to use Faraday's law of electrolysis. The formula is:

Mass (g) = (Current (A) * Time (s)) / (Molar mass (g/mol) * Faraday's constant (C/mol))

Given that the current is 15.0 A and the time is 60.0 minutes (or 3600 seconds), we can use the molar mass of nickel (58.69 g/mol) and Faraday's constant (96,500 C/mol) to calculate the mass:

Mass (g) = (15.0 A * 3600 s) / (58.69 g/mol * 96,500 C/mol) = 16.4 g

Therefore, the answer is Choice B) 16.4 g.

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Rewritten by : Barada

Answer:

B) 16.4

Explanation:

Given that:-

Current, I = 15.0 A

Time, t = 60.0 minutes

Also, 1 minute = 60 seconds

So, t = [tex]60\times 60[/tex] s = 3600 s

F is Faraday constant = 96485 C

Atomic weight of Nickel = 58.69 g/mol

Also, Charge on Ni in [tex]NiCl_2[/tex] = 2

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


Thus, according to the Faraday's Law:-

[tex]W=\frac{EIt}{96485}[/tex]

Where, W is the mass of the metal deposited.

So,

[tex]W=\frac{29.34\times 15\times 3600}{96485}\ g=16.4\ g[/tex]

Weight of Ni metal plated out = 16.4 g