How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below?
CaH₂(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + 2 H₂(g)

Question

Quizplus · Accepted Answer

The balanced chemical equation shows that 1 mole of CaH2 produces 2 moles of H2. The molar mass of CaH2 is 42.09 g/mol. Therefore, the mass of CaH2 required to produce 4.56 L of H2 at 25.0°C and 0.975 atm pressure is:mass of CaH2 = (4.56 L H2) x (1 mol H2 / 22.4 L H2) x (1 mol CaH2 / 2 mol H2) x (42.09 g CaH2 / 1 mol CaH2) = 82 g CaH2

How Many Grams of Calcium Hydride Are Required to Produce