Question

2. a sample of gas of mass 1.245 g occupies a volume of 639 ml at 27.0 oc and 1.00 atm pressure. what is the molar mass of the gas?

Answer 1

The molar mass of the gas is 48 g/mol. The result is obtained by using the ideal gas equation.

What is ideal gas equation?

The gas is ideal when it obeys an equation of state, pV = nRT.

Where

• p = pressure of gas
• V = volume of gas
• n = number of moles
• R = gas constant (0.082057 L.atm.K⁻¹.mol⁻¹)
• T = temperature of gas

It is known as ideal gas law.

The molar mass of a gas can be counted by the following equation.

M = m/n

Where

• M = molar mass of gas
• m = mass of gas

A sample of gas with a mass of 1.245 g occupies a volume of 639 ml at 27.0°C and 1.00 atm pressure. What is the molar mass of the gas?

From that information, we get:

• m = 1.245 g
• V = 639 ml = 0.639 L
• T = 27.0°C = 300.15K
• p = 1.00 atm

The molar mass is M = m/n. Then, the number of moles is n = m/M. We can substitute n value into ideal gas equation.

The molar mass of the gas is

pV = nRT

pV = (m/M) × RT

1.00 × 0.639 = (1.245/M) × 0.082057 × 300.15

0.639 = 30.664/M

M = 30.664/0.639

M = 47.987

M = 48 g/mol

Hence, the molar mass of the gas is 48 g/mol.

Learn more about ideal gas equation here:

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