The density of a gaseous chlorofluorocarbon (CFC) at 23.8 °C and 432 mmHg is 3.23 g/L. What is its molar mass?

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Quizplus · Accepted Answer

The molar mass of the gaseous chlorofluorocarbon can be calculated using the ideal gas law equation rearranged to solve for molar mass (M): $M = \frac{dRT}{P}$, where $d$ is the density of the gas, $R$ is the ideal gas constant (0.0821 L·atm/K·mol), $T$ is the temperature in Kelvin, and $P$ is the pressure in atm. First, convert the temperature to Kelvin (T = 23.8 + 273.15 = 296.95 K) and the pressure to atm (P = 432 mmHg * (1 atm / 760 mmHg) = 0.5684 atm). Then, substitute the values into the equation: $M = \frac{3.23 g/L \times 0.0821 L·atm/K·mol \times 296.95 K}{0.5684 atm} = 139 g/mol$.

The Density of a Gaseous Chlorofluorocarbon (CFC) at 23