Question

A current of 7.11x104 A is passed through an electrolysis cell containing molten NaCl for 6.30 days. (a) How many grams of sodium are produced? (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L

Answer 1

(a) Na⁺ + e^-$\rightarrow$ Na

charge passed = 7.11×10⁴ × 6.30×24×3600 C

= 3.87×10¹⁰C

Number of Faraday's passed = 3.87×10¹⁰/96485

= 4.0111×10⁵ faraday

Mass of sodium deposited = 4.0111×10⁵×22.9898 g

= 9.22145×10⁶ g

= 9.22×10⁶ g. (Answer)

(b) 2Cl^-$\rightarrow$ Cl₂ (g) + 2e^-.   

A current of 2 faraday would produce 1 mole of chlorine gas.

Number of moles chlorine gas produced = 4.0111×10⁵/2

= 2.00555×10⁵ mol

PV = n RT

Volume of gas collected = 2.00555×10⁵mol × 0.0821atm-L/K.mol×273K /1.00atm

= 4.495×10⁶ L

= 4.50×10⁶ L. (Answer)