How much hydrogen will be required to recover 128 g from copper (II) oxide?

Divalent copper oxide is reduced with hydrogen gas when heated. This synthesizes metallic copper and water. This reaction is described by the following equation:

CuO + H2 = Cu + H2O;

Cupric oxide reacts with hydrogen in equal (equivalent) molar amounts. In the course of the reaction, the same equal chemical amounts of copper and water are synthesized.

Let’s find the chemical amount of copper.

To do this, divide the weight of copper by the weight of 1 mole of metal.

M Cu = 64 grams / mol;

N Cu = 128/64 = 2 mol;

The same amount of hydrogen will be required. Let’s calculate the volume of hydrogen. To this end, we multiply the amount of substance by the volume of 1 mole of gas (22.4 liters).

N H2 = 2 mol;

V H2 = 2 x 22.4 = 44.8 liters;