Sixty liters of a gas were collected over water when the barometer read 663 mmhg, and the temperature was 20∘c. what volume would the dry gas occupy at standard conditions? (hint: consider dalton's law of partial pressures.)

Question

Chemistry

Demarion Gallagher

23 November, 23:50

Sixty liters of a gas were collected over water when the barometer read 663 mmhg, and the temperature was 20∘c. what volume would the dry gas occupy at standard conditions? (hint: consider dalton's law of partial pressures.)

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Jeffrey Mcclure · Answer 1

First, let's compute the number of moles in the system assuming ideal gas behavior.

PV = nRT

(663 mmHg) (1atm/760 mmHg) (60 L) = n (0.0821 L-atm/mol-K) (20+273 K)

Solving for n,

n = 2.176 moles

At standard conditions, the standard molar volume is 22.4 L/mol. Thus,

Standard volume = 22.4 L/mol * 2.176 mol = 48.74 L