31.
10.0 g of gas occupies a volume of 2 L at a pressure of 1 atm
and a temperature of 27°C. What is the molar mass of the gas?
a
246.18 g/mol
b
None of the above
C 300.02 g/mol
d 123:09 g/mol



Answer :

To find the molar mass of the gas, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin. First, let's convert the temperature from Celsius to Kelvin: 27°C + 273 = 300 K Next, we need to find the number of moles of the gas using the given mass and molar mass: Given mass = 10.0 g Volume = 2 L Pressure = 1 atm Temperature = 300 K From the ideal gas law, we can rearrange the equation to solve for n: n = (PV) / (RT) n = (1 atm * 2 L) / (0.0821 atm L/mol K * 300 K) n = 0.067 moles Now, we can calculate the molar mass of the gas using the formula: Molar mass = (mass of gas) / (number of moles) Molar mass = 10.0 g / 0.067 mol Molar mass ≈ 149.25 g/mol Therefore, none of the provided options match the calculated molar mass of approximately 149.25 g/mol. Hence, the correct answer would be "None of the above" as the molar mass of the gas does not correspond to the given options.