One of the half-reactions for the electrolysis of water is 2H + (aq) + 2e - → H2 (g) If 0.845 L of H2 is collected at 25°C and 782 mmHg, how many faradays of electricity had to pass through the solution?

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Chemistry

22 November, 04:14

One of the half-reactions for the electrolysis of water is 2H + (aq) + 2e - → H2 (g) If 0.845 L of H2 is collected at 25°C and 782 mmHg, how many faradays of electricity had to pass through the solution?

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Emery · Answer 1

0.0725 faradays of electricity had to be passed through the solution.

Explanation:

Find how many hydrogen moles are produced.

1 mole of any gas consumes 24 liters at room temperature

atmospheric pressure 1 environment is 760 mm Hg

temperature is 25 deg C

so if you reduced the pressure down to 760 mm Hg on that 0.845 liters you've gathered, you would discover the volume expanded to

0.845 x 782/760 = 0.869 liters

which equals to 0.0362 moles (divide by 24)

since every atom of hydrogen required 2 electrons to be made, hence we need 0.0725 moles of electrons or 0.0725 faradays.