Find the mass of hydrogen required to reduce copper from its oxide with a mass of 500 g.

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

CuO + H2 = Cu + H2O;

Cupric oxide reacts with hydrogen in equal molar amounts. At the same time, the same equal amounts of copper and water are synthesized.

Determine 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 = 500/80 = 6.25 mol;

Thus, 6.25 mol of copper oxide can be reduced and 6.25 mol of copper can be obtained.

Let’s calculate the mass and volume of 6.25 mol of hydrogen.

M H2 = 2 grams / mol;

m H2 = 2 x 6.25 = 12.5 grams;

V H2 = 6.25 x 22.4 = 140 liters;