A sample of gas weighs 1.25 g, at 28 C occupying a volume of 2.50 x 10^2 ml and its pressure is 715 torr. What is the molar mass in grams?
Correct answer: A. 131.1
- A. 131.1
- B. 1.311
- C. 1.212
- D. 122.1
Explanation
Mass of gas = 1.25 g The volume of gas = 2.50 x 102 ml= 0.25 L Pressure of gas = 715 torr The temperature of gas = Using the ideal gas law, PV=nRT PV=(m/M)RT M=mRT/PV where, M = Molar mass of gas W = Mass of gas R = gas constant T = temperature of the gas P = Pressure of gas V = Volume of gas Now put all the given values in the above formula, and we get the value of the molar mass of gas. M=(1.25)(62.364)(1.25)/(715)(0.25) M=131.1g/mol
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About Ideal Gas Equation
The ideal gas equation, PV = nRT, relates pressure, volume, amount and absolute temperature when gas particles are assumed to have negligible volume and no intermolecular forces. Applications include finding molar mass, density or an unknown gas variable, with careful use of Kelvin temperature and consistent units, and comparison with real-gas behaviour.
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