Calculate the volume of oxygen required for complete oxidation of 2.8 g of silicon.

Let’s implement the solution:

In accordance with the condition of the problem, we write down the equation of the process:
m = 2.8 g; Xl (O2) -?

Si + O2 = SiO2 – compounds, silicon oxide was formed;

We make calculations:
M (Si) = 28 g / mol;

M (O2) = 32 g / mol.

Determine the amount of the original substance, if the mass is known:
Y (Si) = m / M = 2.8 / 28 = 0.1 mol;

Y (O2) = 0.1 mol since the amount of substances is 1 mol.

We find the volume of O2:
V (O2) = 0.1 * 22.4 = 2.24 L

Answer: you need oxygen with a volume of 2.24 liters.