Final answer:
To calculate the molecular mass of the given gas, convert pressure to atm, volume to L, and temperature to K, then apply the Ideal Gas Law to find moles, and divide the mass of the gas by the number of moles. The molecular mass is determined to be 105.3 g/mol.
Step-by-step explanation:
To calculate the molecular mass of the gas in question, we can use the Ideal Gas Law, which is PV = nRT, where P is the pressure, V is the volume, n is the amount of substance in moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the given values to the appropriate units for these calculations:
- The pressure in torr must be converted to atmospheres: 747.2 torr / 760 torr/atm = 0.98316 atm.
- The volume should be in liters: 1484 mL / 1000 mL/L = 1.484 L.
- The temperature must be in Kelvin: 27.3°C + 273.15 = 300.45 K.
Now, with the values in the correct units, we can rearrange the Ideal Gas Law to solve for n (the number of moles):
n = PV / RT = (0.98316 atm × 1.484 L) / (0.0821 L·atm/(mol·K) × 300.45 K) = 0.05847 mol.
The molecular mass of the gas can now be found by dividing the mass of the gas by the number of moles:
Molecular Mass = mass / n = 6.155 g / 0.05847 mol = 105.3 g/mol.
Assuming ideal gas behavior, the calculated molecular mass is 105.3 g/mol.