A dry gas at a temperature of 67.5 C and a pressure of 882 torr occupies a volume of 242.2 mL. What will be the volume of the gas at a new pressure of 840 tor and 80 C

265 mL is the new volume for the gas

Explanation:

We decompose the Ideal Gases Law in order to find the answer of this question: P. V = n. R. T

We can propose the formula for the 2 situations, where n remains constant.

R refers to 0.082 L. atm/mol. K which is physic constant.

We convert the temperature to Absolute value:

67.5°C + 273 = 340.5 K

80°C + 273 = 353 K

We convert the volume to L → 242.2 mL. 1 L/1000 mL = 0.2422 L

We convert the pressure values to atm:

882 Torr. 1 atm / 760 Torr = 1.16 atm

840 Torr. 1atm / 760 Torr = 1.10 atm

P₁. V₁ / T₁ = P₂. V₂ / T₂ → Let's replace dа ta:

1.16 atm. 0.2422L / 340.5K = 1.10 atm. V₂ / 353 K

(1.16 atm. 0.2422L / 340.5K). 353K = 1.10 atm. V₂

V₂ = 0.291 L. atm / 1.10 atm → 0.2647 L ≅ 265 mL