Calculate the time required in second to deposit 5.85 g Ni from NiCl_2 solution by passing 10 A current (molar mass of Ni = 58.5\ g mol^ -1 )

Question

Quantrex Academy · Accepted Answer

Correct answer: C. 1930

The reaction for the deposition of Ni is:

\text{Ni}^{2+} + 2e^{-} \rightarrow \text{Ni}

Number of moles of Ni deposited

= \dfrac{5.85}{58.5} = 0.1 \text{ mol}

Since

1 \text{ mole}

of Ni requires

2 \text{ moles}

of electrons, the total charge required is:

Q = 0.1 \times 2 \times 96500 = 19300 \text{ C}

Using the formula

Q = I \times t

:

19300 = 10 \times t

t = 1930 \text{ s}

Answer:

1930

Calculate the time required in second to deposit 5.85 g Ni from...