#### Question

The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol^{-1}) from sodium ions is -

- 2098
- 96500
- 193000
- 4196

#### Solution

(d) 4196

Moles of Na = 1.00/23.0 = 0.0435

Cathode-half reaction will be

Na^{+} + 1 e^{-} → Na

It states that for every one Faraday consumed, one mole of Na is liberated.

This means to get 0.0435 moles, we need to use 0.0435 Faraday.

We know that

1 Faraday = 96500 coulomb

0.0435 Faraday = 4197.75 coulomb

So, the nearest option is **4196**.

Is there an error in this question or solution?

#### APPEARS IN

Solution The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is Concept: Electrolytic Cells and Electrolysis - Introduction.