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A 23.6 g sample of an unknown gas occupies a volume of 12.0 L at standard temperature and pressure. What is the molecular mass (molar mass) of this gas?

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Lanuel

The molecular mass (molar mass) of this gas is equal to 44.08 g/mol.

Given the following data:

  • Mass = 23.6 grams
  • Volume = 12.0 Liters
  • Standard temperature = 273 K
  • Standard pressure = 1 atm.

To calculate the molecular mass (molar mass) of this gas, we would use the ideal gas law equation;

[tex]PV=\frac{MRT}{MM}[/tex]

Where;

  • P is the pressure.
  • V is the volume.
  • M is the mass of substance.
  • MM is the molar mass of a substance.
  • R is the ideal gas constant.
  • T is the temperature.

Making MM the subject of formula, we have:

[tex]MM = \frac{MRT}{PV} \\\\MM = \frac{23.6\times 0.0821 \times 273}{1 \times 12}\\\\MM = \frac{528.95}{12}[/tex]

Molar mass, MM = 44.08 g/mol.

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