In the electrolysis of water, how long will it take to produce 140.0 L of H2 at 1.0 atm and 273 K using an electrolytic...

Question

Question

In the electrolysis of water, how long will it take to produce 140.0 L of H2 at 1.0 atm and 273 K using an electrolytic cell

science chemistry

Answer 1

Answer #1

Reaction at cathode :

2H₂O(l) + 2e^- $\rightarrow$ H₂(g) + 2 OH^-(aq)

PV = nRT

n =1.0atm × 140.0L /(0.0821atm-L/K.mol × 273K)

= 6.2463 mol

2 mole of electrons or 2 Faradays are needed to release 1 mole of H₂ gas.

Number of faraday passed to produce 6.2463mol of hydrogen = 2 × 6.2463 = 12.4926 faraday

Q = I×t

Time required to produce the desired hydrogen = 12.4926 × 96485 / 0.2300 = 5240638.371 second

= 5240638.371/(3600×24)

= 60.66days (answer)

Answer 2

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