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?

Question

Chemistry

Kael

15 August, 16:24

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?

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Answers (1)

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Giovani Underwood · Answer 1

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)