Question

The quantity of electricity required to deposit 1.15 g of sodium from molten NaCl (Na = 23, Cl = 35.5) is ______.

Options

• 1 F

• 0.5 F

• 0.05 F

• 1.5 F

Answer 1

The quantity of electricity required to deposit 1.15 g of sodium from molten NaCl (Na = 23, Cl = 35.5) is 0.05 F.

Explanation:

The reduction reaction in molten NaCl is:

\[\ce{Na+ + e- -> Na}\]

So, 1 mole (23 g) of Na requires 1 Faraday (F) of charge.

Now, we are given:

Mass of Na deposited = 1.15 g

Atomic mass of Na = 23 g/mol

Number of gram equivalents = `1.15/23`

= 0.05

Since 1 gram equivalent = 1 Faraday, then Charge required = 0.05 F.