what volume of hydrogen gas at STP is required to completely react with excess of oxygen to form 0.9 grams of water?

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Solution

H₂ + 1/2 O₂ → H₂O
1 mole of hydrogen result into the formation of 1 mole of water.
Mass of Water formed = 0.9 g
Number of moles of water = mass/molecular mass = 0.9/18 = 0.05 moles
So, 0.05 moles of hydrogen were needed to form 0.9 g water.
1 mole of any gas occupy volume = 22.4 L
0.05 moles of Hydrogen will have volume = 22.4 * 0.05 = 1.12 L

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