1. Convert Temperature to Kelvin:
* T(K) = T(°C) + 273.15
* T(K) = 15°C + 273.15 = 288.15 K
2. Use the Ideal Gas Law:
* PV = nRT
* P = Pressure (atm) = 0.892 atm
* V = Volume (L) = 5.00 L
* n = Number of moles
* R = Ideal gas constant (0.0821 L·atm/mol·K)
* T = Temperature (K) = 288.15 K
3. Solve for the Number of Moles (n):
* n = (PV) / (RT)
* n = (0.892 atm * 5.00 L) / (0.0821 L·atm/mol·K * 288.15 K)
* n ≈ 0.199 mol
4. Calculate the Mass of the Gas:
* Density = Mass / Volume
* Mass = Density * Volume
* Mass = 1.22 g/L * 5.00 L = 6.10 g
5. Determine the Molecular Weight:
* Molecular Weight (M) = Mass / Moles
* M = 6.10 g / 0.199 mol
* M ≈ 30.7 g/mol
Therefore, the molecular weight of the gas is approximately 30.7 g/mol.
