Answer:
- Mole fraction of Chlorine Pentafluoride
= 0.265
- Partial Pressure of Chlorine Pentafluoride
= 16.05 kPa
- Mole fraction of Sulfur Hexafluoride
= 0.735
- Partial Pressure of Sulfur Hexafluoride
= 44.53 kPa
Total Pressure exerted by the gases = 60.58 kPa
Explanation:
First of, we calculate the number of moles of each gas present.
Number of moles = (Mass)/(Molar Mass)
For ClF₅
Mass = 4.28 g
Molar Mass = 130.445 g/mol
number of moles of Chlorine Pentafluoride
= (4.28/130.445) = 0.0328 moles
For SF₆
Mass = 13.3 g
Molar Mass = 146.06 g/mol
number of moles of Sulfur Hexafluoride
= (13.3/146.06) = 0.0911 moles
Total number of moles present = 0.0328 + 0.0911 = 0.1239 moles.
Using the ideal gas equation
PV = nRT
P = total pressure in the tank = ?
V = volume of the tank = 5.00 L = 0.005 m³
R = molar gas constant = 8.314 J/mol.K
T = temperature of the tank = 20.9°C = 294.05 K
n = total number of moles present = 0.1239 moles
P × 0.005 = (0.1239 × 8.314 × 294.05)
P = 60,580.45 Pa = 60.58 kPa.
- Mole fraction of a particular component of interest = (number of moles of the component of interest) ÷ (total number of moles)
- Partial Pressure of a particular component of interest = (mole fraction of that component of interest) × (total pressure)
This is Dalton's law of Partial Pressure.
- Mole fraction of Chlorine Pentafluoride
= (0.0328/0.1239) = 0.265
- Partial Pressure of Chlorine Pentafluoride
= 0.265 × 60.58 = 16.05 kPa
- Mole fraction of Sulfur Hexafluoride
= (0.0911/0.1239) = 0.735
- Partial Pressure of Sulfur Hexafluoride
= 0.735 × 60.58 = 44.53 kPa
Total Pressure exerted by the gases = 16.04 + 44.53 = 60.58 kPa
Hope this Helps!!!
is the pressure inside the container.
is the volume of the container.
is the number of moles of particles (molecules, or atoms in case of noble gases) in the gas.
is the ideal gas constant.
is the absolute temperature of the gas.