How much oxygen is consumed in the oxidation of copper if copper oxide weighing 1.6 g is formed?

Metallic copper reacts with oxygen to form oxide. The reaction is described by the following chemical equation:

Cu + ½ O2 = CuO ↑;

Let’s determine the chemical amount of copper oxide. To do this, divide the mass of the available substance by the weight of 1 mole.

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

N CuO = 1.6 / 80 = 0.02 mol;

To obtain such an amount of copper oxide, it is necessary to take 2 times less oxygen.

Let’s calculate the weight and volume of oxygen.

To find the weight, we multiply the amount of the substance by the weight of 1 mole of the substance.

M O2 = 16 x 2 = 32 grams / mol;

m O2 = 0.02 / 2 x 32 = 0.32 grams;

To find the volume of oxygen, we multiply the amount of the substance by the volume of 1 mole of gas (which is 22.4 liters).

m O2 = 0.02 / 2 x 22.4 = 0.24 liters;