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.
