How long will it take to collect 1.0 L of H₂ (g) at STP in the electrolysis of 2.0 M HCl with a current of 4.25 A?

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Quizplus · Accepted Answer

At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 L. The gas in question, H₂, is a fictional representation, but for the purpose of this calculation, we can treat it as a real gas. The electrolysis of HCl produces hydrogen gas at the cathode and chlorine gas at the anode. However, since the question specifically asks about the collection of a gas without specifying which, and given the formula provided seems to be a placeholder, we'll proceed with the calculation for hydrogen gas as an example, assuming a similar molar volume.The amount of charge (Q) required to produce 1 mole of hydrogen gas (H2) is based on Faraday's laws of electrolysis. For H2, 2 moles of electrons are required to produce 1 mole of H2 gas.$$ Q = n \times F $$Where $ n $ is the amount of substance in moles, and $ F $ is Faraday's constant (96485 C/mol).Since 1 mole of H2 occupies 22.4 L at STP, to collect 1.0 L of gas, we need $\frac{1.0}{22.4}$ moles of H2.$$ n = \frac{1.0}{22.4} \approx 0.04464 \text{ moles} $$Since 2 moles of electrons are required per mole of H2, the total charge needed is:$$ Q = 0.04464 \times 2 \times 96485 \approx 8600 \text{ C} $$Given a current of 4.25 A (where current $ I = \frac{Q}{t} $), the time $ t $ can be calculated as:$$ t = \frac{Q}{I} = \frac{8600}{4.25} \approx 2023.5 \text{ seconds} $$Converting seconds to minutes:$$ \frac{2023.5}{60} \approx 33.725 \text{ minutes} $$Thus, the closest answer is 34 minutes.

How Long Will It Take to Collect 1