Question

what is the volume of oxygen produced when acidified water is electrolysed by 1.50 A for 30 min?

Answer 1

0.036 liters is the volume of oxygen produced when acidified water is electrolysed.

Explanation:

The quantity of current passed = 1.50 × 30 × 60 = 2700

When converting into faraday = $\frac{2700}{96500}$ = 0.03

The ratio of hydrogen and oxygen produced is 2 : 1

• On passing 1 faraday of electricity 1 mole of hydrogen and 0.5 mole of oxygen is produced.
• On passing 0.03 faraday of electricity 0.03 mole of hydrogen and 0.015 mole of oxygen is produced. 1 mole of any gas = 22.4

Therefore, the volume of hydrogen produced at STP = 0.03 × 22.4 = 0.672 liters.

The volume of oxygen produced at STP = 0.015 × 22.4 = 0.336 liters.

Thus the volume of oxygen produced when acidified water is electrolysed by 1.50 A is 0.036 liters.

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