Determine the amount of hydrogen required for the complete reduction of 0.2 mol of copper (II) oxide.

Copper oxide is reduced with hydrogen gas. During the reaction, metallic copper and water are synthesized. The reaction is described by the following chemical reaction equation:

CuO + H2 = Cu + H2O;

Cupric oxide reacts with hydrogen in equal (equivalent) molar amounts. In this case, the same equal amounts of metallic copper and water are synthesized.

In order to carry out the reduction of 0.2 mol of copper oxide, 0.2 mol of hydrogen is required.

Let’s define its volume. To do this, multiply the amount of substance and the volume of 1 mole of gas, which is 22.4 liters.

V H2 = 0.2 x 22.4 = 4.48 liters;