How many grams of copper will be obtained when a 100 g sample containing 90% copper (II) oxide is reduced with hydrogen?

Divalent copper oxide is reduced with hydrogen gas when heated. This synthesizes metallic copper and water. 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 the course of the reaction, the same equal chemical amounts of copper and water are synthesized.

Let’s calculate the chemical amount of copper oxide.

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

M CuO = 64 + 16 = 80 grams / mol;

N CuO = 100 x 0.9 / 80 = 1.125 mol;

Thus, it is possible to carry out the reduction of 1.125 mol of copper oxide and obtain 1.125 mol of copper.

Its mass will be equal to:

M Cu = 64 grams / mol;

m Cu = 64 x 1.125 = 72 grams;