Question

When solid copper (II) oxide is heated in the presence of hydrogen gas, the products are copper metal and water vapor according to the following balanced equation. CuO (s) + H₂ (g) → Cu (s) + H₂O (g). In order to obtain 17 g of copper metal, how many grams of hydrogen gas must react?

Answer 1

To obtain 17 g of copper metal, approximately 0.5401 g of hydrogen gas must react.

Step-by-step explanation:

To determine the amount of grams of hydrogen gas needed to react and produce 17 g of copper metal, we need to use the stoichiometry of the balanced equation. According to the balanced equation, 1 mole of CuO reacts with 1 mole of H₂ to produce 1 mole of Cu and 1 mole of H₂O.

The molar mass of Cu is 63.546 g/mol. Therefore, 17 g of Cu is equal to 17 g / (63.546 g/mol) = 0.2677 mol of Cu. Since the mole ratio between Cu and H₂ is 1:1, we need 0.2677 mol of H₂.

The molar mass of H₂ is 2.016 g/mol. Therefore, the mass of 0.2677 mol of H₂ is 0.2677 mol * (2.016 g/mol) = 0.5401 g of H₂.