Question

What is the molar mass of a gas with a density of 4.03 g/L at –73EC and 1,140 torr?

Answer 1

44.1 g/mol

Step-by-step explanation:

Step 1: Convert the temperature to the Kelvin scale.

We will use the following expression.

K = °C + 273.15

K = -73°C + 273.15

K = 200 K

Step 2: Convert the pressure to atm

We will use the relationship 1 atm = 760 torr.

`1,140torr * (1atm)/(760torr) = 1.50 atm`

Step 3: Calculate the molar mass of the gas

We will use the following equation derived from the ideal gas equation.

`P * M = \rho * R * T\\M = (\rho * R * T)/(P) = (4.03g/L * (0.0821atm.L)/(mol.K) * 200K)/(1.50atm) = 44.1 g/mol`