One mole of any gas has a volume of 22.4 L at STP. What are the molecular masses of the followi

step 1 So we have the ideal gas law which is pv equals to an r t where r is 0 .08 and n is number of mo

One mole of any gas has a volume of 22.4 L at STP. What are...

One mole of any gas has a volume of $22.4 \mathrm{~L}$ at STP. What are the molecular masses of the following gases, and what are their densities in grams per liter at STP?
(a) $\mathrm{CH}_{4}$
(b) $\mathrm{CO}_{2}$
(c) $\mathrm{O}_{2}$

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Key Concepts

Gas Density Calculation

Gas density at STP can be determined by dividing the molecular mass by the molar volume (22.4 liters). This calculation links the microscopic properties of molecules with the observable macroscopic density, enabling the comparison of different gases under the same conditions.

Molecular Mass

Molecular mass is the sum of the atomic masses of the constituent atoms in a molecule, measured in grams per mole. It is crucial for converting between the number of moles and the mass of a chemical substance.

Mole Concept

The mole is a fundamental unit in chemistry that represents 6.022×10^23 particles of a substance. It connects the macroscopic amounts we measure with the microscopic scale of individual atoms or molecules, enabling quantitative chemical analysis.

Standard Temperature and Pressure (STP)

STP refers to a set of conditions, typically 0°C and 1 atm pressure, under which one mole of an ideal gas occupies 22.4 liters. This standardized condition simplifies calculations and comparisons of gas volumes and densities.

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