Calculate the mass of sulfur oxide (6), which was formed during the oxidation of sulfur oxide (4)

Calculate the mass of sulfur oxide (6), which was formed during the oxidation of sulfur oxide (4) with a mass of 16 g, if the yield of the reaction product is 80% of the theoretically possible.

In accordance with the condition of the problem, we write the equation:
2SO2 + O2 = 2SO3 – redox reaction, sulfur oxide was obtained (6);
Let’s calculate the molar masses of substances:
M (SO2) = 64 g / mol;
M (SO3) = 80 g / mol.
Let us determine the amount of moles of sulfur oxide (4), if the mass is known:
Y (SO2) = m / M = 16/64 = 0.25 mol;
According to the equation, the amount of moles of sulfur oxide (4) and sulfur oxide (6) are equal to 2 moles, which means that Y (SO3) = 0.25 moles.
Find the theoretical mass of sulfur oxide (6):
m (SO3) = Y * M = 0.25 * 80 = 20 g.
Let us calculate the practical mass of sulfur oxide (6):
W = m (practical) / m (theoretical) * 100;
m (practical) = 0.8 * 20 = 16g
Answer: the mass of the highest sulfur oxide is 16 g.