What volume of hydrogen gas at STP would be liberated by action of 50 mL of of 50% purity

Question

What volume of hydrogen gas at STP would be liberated by action of 50 mL of $H_{2} {SO}_{4}$ 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. [2026]

Smart Achievers · Accepted Answer

(3)

$Mass of impure H_{2} S O_{4} sample$

$= density \times volume = 1.3 {g mL}^{- 1} \times 50 mL = 65 g$

$Mass of pure H_{2} S O_{4} = 0.5 \times 65 g = 32.5 g$

$Moles of pure H_{2} S O_{4}$

$= \frac{Given mass}{Molar mass} = (\frac{32.5}{98}) mol = 0.33 mol$

$Moles of zinc = \frac{Given mass}{Molar mass} = (\frac{20}{65}) mol = 0.3077 mol$

$H_{2} S O_{4} + Z n \to Z n S O_{4} + H_{2}$

$As per reaction stoichiometry, 0.3077 mol of Zn react with$

$0.3077 mol H_{2} S O_{4} to form 0.3077 mol H_{2} gas.$

$Volume of H_{2} gas at STP = 0.3077 \times 22.4 L = 6.892 L$

Solution

Q.
What volume of hydrogen gas at STP would be liberated by action of 50 mL of $H_{2} {SO}_{4}$ 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. [2026]

1 5.824 L

2 7.428 L

3 6.892 L

4 8.375 L

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