A sample of 4.50 g of diatomic oxygen (O2) occupies a volume of 15.0 L at a temperature of 203 K and a pressure of 5.0 atm. What will be the volume of the same sample if the pressure increases to 15.0 atm and the temperature is raised to 303 K?

V = 0.23 Lt

Explanation:

dа ta: O₂ 4.50 g = 0.14 mol (considering a molecular mass of 32 g for O₂)

V₁ = 15.0 Lt, T₁ = 203 K, P₁ = 5.0 atm

V₂ = ?, T₂ = 303 K, P₂ = 15.0 atm

If we consider that this gas beahves as an ideal gas, then:

PV = nRT

V = nRT/P

V₂ = nRT₂/P₂, where R gas constant = 0.082 Lt*atm/K*mol

V₂ = (0.14x0.082x303) / 15.0 ⇒ V₂ = 0.23 Lt

Which is consistent, considering that the gas is subjected to a high pressure (from 5 atm to 15 atm), its volume should decrease (from 15 Lt to 0.23 Lt)