Question

If the density of an ideal gas at stp if found to be 0.0902 g/l, what is its molar mass?

Answer 1

Answer: The molar mass of the gas is 2.02 grams.

Explanation:

We are given:

Density of gas = 0.0902 g/L

At STP conditions:

1 mole of gas occupies 22.4 L of volume

And 1 mole of a substance is known as the molecular mass or molar mass of that substance.

To calculate the mass of gas, we use the equation:

$\text{Density of gas}=\frac{\text{Mass of gas}}{\text{Volume of gas}}$

Putting values in above equation, we get:

$0.0902g/L=\frac{\text{Mass of gas}}{22.4L}\\\\\text{Mass of gas}=2.02g$

Hence, the molar mass of the gas is 2.02 grams.

Answer 2

The molar mass of the ideal gas is determined as 2.02 g.

The given parameters;

• density of the ideal gas, ρ = 0.0902 g/l

The density of any fluid is obtained by diving the mass of the fluid by its volume;

$\rho = \frac{mass}{volume}$

• Volume of an ideal gas at stp is 22.4 L/mol

The molar mass of the ideal gas is calculated as follows;

mass = density x volume

mass = 0.0902 x 22.4

mass = 2.02 g

Thus, the molar mass of the ideal gas is determined as 2.02 g.

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