Question

How many coulombs of electricity is required to produce 1g of sodium metal by reduction of sodium ion? 

Answer 1

To calculate the coulombs of electricity required to produce 1g of sodium metal by the reduction of sodium ion, we use Faraday's Law of electrolysis.

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

This shows that 1 mole of Na⁺ requires 1 mole of electrons (1 Faraday = 96,500 C).

Calculate Moles of Na in 1g

Molar mass of Na = 23 g/mol

Moles of Na in 1g = `1/23` = 0.0435 moles

Since 1 mole of Na requires 96,500 C, for 0.0435 moles: 

Charge required = 0.0435 × 96,500

= 4,197.75 C