How much hydrogen is needed to reduce copper from 80 g of copper oxide (2) containing 20% impurities?

The reduction of copper from its oxide is described by the following chemical reaction equation:

CuO + H2 = Cu + H2O;

In accordance with the coefficients of the chemical reaction equation, the reduction of one mole of copper oxide requires one mole of hydrogen.

Find the amount of substance contained in 80 grams of copper oxide containing 20% ​​impurities. To do this, we divide the mass of pure oxide by its molar mass.

The pure oxide mass will be 80 x 0.8 = 64 grams.

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

N CuO = 64/80 = 0.8 mol;

The amount of hydrogen required is also 0.8 mol.

Under normal conditions, one mole of ideal gas takes up a volume of 22.4 liters.

The volume of hydrogen will be:

V H2 = 0.8 x 22.4 = 17.92 liters;