What is the gas temperature after the expansion (in ∘C) ? Five grams of nitrogen gas at an initial pressure of 3.0 atm and at 20∘C undergo an isobaric expansion until the volume has tripled.

Gas temperature after the expansion = T₂ = 879.45 K = 606.3°C

Explanation:

For ideal gases, the general gas law is given by

(P₁V₁/T₁) = (P₂V₂/T₂)

P₁ = 3.0 atm

V₁ = V

T₁ = 20°C = 293.15 K

P₂ = P₁ = 3.0 atm (since it's an isobaric process; constant pressure)

V₂ = 3V

T₂ = ?

(3*V/293.15) = (3*3V) / T₂

T₂ = (3*3V*293.15) / (3*V)

T₂ = 879.45 K = 606.3°C