Answer -
Given,
Volume of Flask = 9.02 L
Temperature = 24C or 297.15 K [0°C + 273.15 = 273.15K]
mass of Krypton = 33.5 g
molar mass of Krypton = 83.798 u
mass of Oxygen gas = 8.39 g
molar mass of O2 = 32 u
Partial Pressure of Oxygen Gas = ?
Total Pressure = ?
According to Dalton's Law,
Partial Pressure = Mole Fraction * Total Pressure
Also,
Molar Fraction = Moles/ Total Moles
Partial Pressure = (Moles/ Total moles) * Total Pressure --------A
Also,
Moles = Mass/Molar Mass
Moles of Krypton = 33.5 g/83.798 u
Moles of Krypton = 0.4 mol
Moles of O2 = 8.39g /32 u
Moles of O2 = 0.26 mol
Total Moles = Moles of Krypton + Moles of Oxygen gas
Total Moles = 0.4 mol + 0.26 mol = 0.66 mol
Now,
We know that,
PV = nRT
where, P = Pressure
V = Volume
n = mole
R = Gas Constant (0.082057 L atm K−1mol−1)
T = Temperature in K
Put the values,
Ptotal * V = ntotal *R*T
Ptotal * 9.02 L = 0.66 mol *0.082057 L atm K−1mol−1 *297.15 K
Ptotal = 1.78 atm [Answer]
Put the values in A,
Partial Pressure = (Moles/ Total moles) * Total Pressure
Partial Pressure of Oxygen gas = (0.26 mol/ 0.66 mol) * 1.78 atm
Partial Pressure of Oxygen gas = 0.70 atm [Answer]
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