In the electrolysis of water the volume of oxygen collected is 2.24 L at STP. How many grams of hydrogen gas are collected?
Question
In the electrolysis of water the volume of oxygen collected is 2.24 L at STP. How many grams of hydrogen gas are collected?
Solution
Sure, here's how you can solve this problem:
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First, we need to understand that in the electrolysis of water, the reaction is 2H2O -> 2H2 + O2. This means that for every molecule of O2 produced, two molecules of H2 are produced.
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The volume of gases at STP is proportional to the number of molecules (or moles) of the gas. So, if we have 2.24 L of O2, we will have twice that volume of H2, which is 2.24 L * 2 = 4.48 L.
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At STP, 1 mole of any gas occupies 22.4 L. So, the number of moles of H2 is 4.48 L / 22.4 L/mole = 0.2 moles.
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The molar mass of H2 is approximately 2 g/mole. So, the mass of H2 produced is 0.2 moles * 2 g/mole = 0.4 g.
So, 0.4 grams of hydrogen gas are collected.
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