If you double the volume of a sample of gas and then doubled the volume again without changing its pressure, how would this absolute temperature of the gas be affected

Explanation:

Increasing Volume while maintaining constant pressure requires a proportional increase in Temperature so the gas pressure will be maintained as constant.

Consider...

V₁ = V₁     V₂ = 4V₁

T₁ = T₁      T₂ = ?

Charles Law => T ∝ V at constant P ... that is, increasing temperature generates a proportional increase in volume to maintain constant pressure.

Empirical Charles Law Relation is ...

V₁/T₁ = V₂/T₂ => T₂ = T₁(V₂/V₁) = T₁(4V₁/V₁) = 4T₁

Increasing Volume of a gas by 4 times requires a 4 times increase in absolute temperature in order to maintain constant pressure.

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