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 data:

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

r just means there's a number of carbon in teh chain. for example rcooh means that after x number of carbon, the chain ends with cooh.

explanation:

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