1. Convert Units:
* Temperature (T): Convert Celsius to Kelvin: 33°C + 273.15 = 306.15 K
* Pressure (P): Convert kPa to atmospheres (atm): 199 kPa * (1 atm / 101.325 kPa) = 1.96 atm
2. Use the Ideal Gas Law:
The Ideal Gas Law is: PV = nRT
Where:
* P = Pressure (in atm)
* V = Volume (in liters)
* n = Number of moles
* R = Ideal gas constant (0.0821 L⋅atm/mol⋅K)
* T = Temperature (in Kelvin)
3. Solve for 'n' (number of moles):
Rearrange the Ideal Gas Law to solve for 'n':
n = PV / RT
4. Plug in the values and calculate:
n = (1.96 atm * 4.67 L) / (0.0821 L⋅atm/mol⋅K * 306.15 K)
n ≈ 0.364 moles
Therefore, the 4.67 L sample of gas contains approximately 0.364 moles.
