If a 0.614 g sample of a gas maintains a pressure of 238 mm Hg when contained in a 1.0 L flask at 0.0°C,what is molar mass of the gas?

Question

Quizplus · Accepted Answer

Using the ideal gas law, PV = nRT, and rearranging for molar mass (M = mRT/PV), where m = mass of gas, R = ideal gas constant (0.0821 L·atm/mol·K), P = pressure in atm (238 mm Hg converted to atm is 238/760), V = volume in liters, and T = temperature in Kelvin (273 K for 0.0°C), we can calculate the molar mass. Plugging in the values, we find the molar mass to be approximately 44 g/mol.

If a 0614 G Sample of a Gas Maintains a Pressure of Pressure