A sample of nitrogen gas had a volume of 500. ml, a pressure in its closed container of 740 torr and a temperature 25 degrees c of what was the new volume of the gas when the temperature was changed to and the new pressure was

Question:

A sample of nitrogen gas had a volume of 500mL, a pressure in its closed container of 740 torr and a temperature of 25°c. what was the volume of gas when the temperature was changed to 50°c and the new pressure was 760 torr?

Answer:

Data Given:

V ₁ = 500 mL

P₁ = 740 torr

T₁ = 25 °C + 273 = 298 K

V₂ = ?

P₂ = 760 torr

T₂ = 50 °C + 273 = 323 K

Solution:

Let suppose the gas is acting Ideally, then According to Ideal Gas Equation,

P₁ V₁ / T₁ = P₂ V₂ / T₂

Solving for V₂,

V₂ = (P₁ V₁ T₂) : (T₁ P₂)

Putting Values,

V₂ = (740 torr * 500 mL * 323 K) : (298 K * 760 torr)

V₂ = 527.68 mL