Calcium hydride (\text{CaH}_2) reacts vigorously with water to produce calcium hydroxide a… — JAMB UTME

Calcium hydride ( $\text{CaH}_2$ ) reacts vigorously with water to produce calcium hydroxide and hydrogen gas. What volume of dry hydrogen gas, in $\text{dm}^3$ , measured at standard temperature and pressure (s.t.p.), is liberated when $10.5\text{ g}$ of pure calcium hydride reacts completely with excess water?

[Relative atomic masses: $\text{Ca} = 40$ , $\text{H} = 1$ ; Molar volume of gas at s.t.p. = $22.4\text{ dm}^3\text{ mol}^{-1}$ ]

Answer: 11.2 dm^3

Answer

The volume of dry hydrogen gas liberated at s.t.p. is 11.2 dm³.

Calcium hydride reacts with water according to the reaction CaH₂ + 2H₂O → Ca(OH)₂ + 2H₂. Given 10.5 g of CaH₂ (molar mass 42 g/mol), there are 0.25 moles of CaH₂. Based on the 1:2 stoichiometric ratio, 0.50 moles of H₂ gas are generated. Multiplying by the molar volume at s.t.p. (22.4 dm³/mol) yields 11.2 dm³.

Step-by-Step Solution

Write the balanced chemical equation for the reaction of calcium hydride with water

CaH₂ + 2H₂O → Ca(OH)₂ + 2H₂

Establishing the stoichiometric mole ratio between the reactant CaH₂ and the product H₂ gas.

Calculate the molar mass of CaH₂

42 g/mol

Molar mass is required to convert the given mass of CaH₂ into moles.

Determine the amount of CaH₂ in moles

0.25 mol

Moles = Mass / Molar mass = 10.5 g / 42 g/mol.

Calculate the moles of H₂ gas liberated using the 1:2 stoichiometric ratio

0.50 mol

1 mole of CaH₂ produces 2 moles of H₂ gas.

Calculate the volume of H₂ gas produced at standard temperature and pressure (s.t.p.)

11.2 dm³

Volume at s.t.p. = Moles × Molar volume at s.t.p. = 0.50 mol × 22.4 dm³/mol.

Key Concept

Laboratory and industrial preparation of hydrogen using metal hydrides and mole-volume stoichiometric calculations at s.t.p.

Estimated Time:2m 0s

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