0.043 mol of a gas weighs 1.892 g. what is the density (in g/l) of this gas at 0.0°c and 9.55 psi? (1.0 atm = 14.7 psi)

1·276 g/L

Explanation:

Given

Number of moles of gas = 0·043

Mass of the gas = 1·892 g

Temperature of the gas = 273 K

Pressure of the gas = 0·65 atm

Assuming that the gas is ideal

Ideal gas equation is P × V = n × R × T

where

P is the pressure of the gas

V is the volume occupied by the gas

n is the number of moles of the gas

R is the ideal gas constant

T is the temperature of the gas

Let the volume of the gas be V L

From ideal gas equation

0·65 × V = 0·043 × 0·0821 ×273

∴ V = 1·483 L

Density is defined as mass per unit volume

Let the density of the gas be d g/L

∴ d = (mass of the gas) ÷ (volume of the gas)

d = 1·892 ÷ 1·483

∴ d ≈ 1·276 g/L

∴ Density of the gas at the given conditions is 1·276 g/L

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