What volume of hydrogen gas at STP would be liberated by action of 50 mL of H_2SO_4 of 50\% purity (density = 1.3 g mL ^ -1 ) on 20 g of zinc ? Given : Molar mass of H, O, S, Zn are 1, 16, 32, 65 g mol ^ -1 respectively.

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Correct answer: C. 6.892 L

Mass of H_2SO_4 solution = 50 1.3 = 65 g Mass of pure H_2SO_4 = 65 50 100 = 32.5 g Moles of H_2SO_4 = 32.5 98 0.3316 mol Moles of Zn = 20 65 0.3077 mol The balanced chemical equation is: Zn + H_2SO_4 ZnSO_4 + H_2 Since the moles of Zn are less than the moles of H_2SO_4, Zn is the limiting reagent. Moles of H_2 produced = Moles of Zn = 20 65 mol Volume of H_2 gas at STP = 20 65 22.4 L = 6.892 L Answer: 6.892 L

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