Question

A gas collected from a reaction has a mass of 1.211 g and occupies a volume of 0.677 L. The temperature in the laboratory is 296 K, and the air pressure is 0.987 atm. Calculate the molar mass of the gas.

23.7 g/mol
44.0 g/mol
58.5 g/mol
82.3 g/mol

Answer 1

Answer: 44.0 g/mol

Explanation:

$M=m.RT/PV$

M=1.211*0.082*296/ 0.987*0.677

M= 44 g/mol

Answer 2

A gas collected from a reaction has a mass of 1.211 g and occupies a volume of 0.677 L. The temperature in the laboratory is 296 K, and the air pressure is 0.987 atm  the molar mass of the gas 23.7 g/mol. option A is correct.

What is gas law?

The universal gas law given by Boyle, Charles , Avogadro and Gauss known as combined gas law with respect to temperature, volume and pressure using universal gas constant and number of moles.

According to universal gas equation or combined gas equation

          P V = n R T

where , P = pressure

             V = volume

              n = number of moles

              R = universal gas constant = 8.313

               T = temperature

n = W / M.M

W = weight

M.M = molar mass

substituting the value in the equation

0.987 × 0.677 = 1.211 / M.M × 8.313 × 296

M.M = 23.7 g/mol

Therefore, gas collected from a reaction has a mass of 1.211 g and occupies a volume of 0.677 L. The temperature in the laboratory is 296 K, and the air pressure is 0.987 atm  the molar mass of the gas 23.7 g/mol. option A is correct.

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