If a gas has a volume of 1000 ML at a temperature of 23°C and a pressure of 100 mmhg, what is it's volume under standard conditions of temperature and pressure?

Question

Reginald Bass

Chemistry

10 October, 14:53

If a gas has a volume of 1000 ML at a temperature of 23°C and a pressure of 100 mmhg, what is it's volume under standard conditions of temperature and pressure?

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Answers (1)

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Essence Irwin · Answer 1

119.7 mL.

Explanation:

From the general law of ideal gases:

PV = nRT.

where, P is the pressure of the gas.

V is the volume of the container.

n is the no. of moles of the gas.

R is the general gas constant.

T is the temperature of the gas (K).

For the same no. of moles of the gas at two different (P, V, and T):

P₁V₁/T₁ = P₂V₂/T₂.

P₁ = 100.0 mmHg, V₁ = 1000.0 mL, T₁ = 23°C + 273 = 296 K. P₂ = 1.0 atm = 760.0 mmHg (standard P), V₂ = ? mL, T₂ = 0.0°C + 273 = 273.0 K (standard T).

∴ V₂ = (P₁V₁T₂) / (T₁P₂) = (100.0 mmHg) (1000.0 mL) (273.0 K) / (296 K) (760.0 mmHg) = 121.4 mL.