How many kilograms of phosphorus (V) oxide should be formed during the combustion of 6.2 kg of phosphorus?

Let’s write the reaction equation:

4P + 5O2 = 2P2O5

Let’s find the amount of phosphorus substance:

v (P) = m (P) / M (P) = 6.2 / 31 = 0.2 (kmol).

According to the reaction equation, from 4 moles of P, 2 moles of P2O5 are formed, therefore:

v (P2O5) = v (P) * 2/4 = 0.2 * 2/4 = 0.1 (kmol).

Thus, the mass of the resulting phosphorus oxide (V):

m (P2O5) = v (P2O5) * M (P2O5) = 0.1 * 142 = 14.2 (kg).

Answer: 14.2 kg.