Answer:
The partial pressure of krypton in the flask is 0.59 atm and the total pressure in the flask is 1.39 atm
Explanation:
This must be solved with the Ideal Gas Law equation.
First of all we need the moles or Ar and Kr in the mixture
Moles = Mass / Molar mass
Molar mass Ar 39.95g/m
Moles Ar = 6.18 g/39.95 g/m → 0.154 moles
Molar mass Kr 83.8 g/m
Moles Kr = 9.66 g/ 83.8g/m → 0.115 moles
Total moles in the mixture: 0.154 moles + 0.115 moles = 0.269moles
Now, we have the total moles, we can calculate the total pressure.
P . V = n . R . T
(T° in K = T° in C + 273)
P. 5.38L = 0.269mol . 0.082 L.atm/mol.K . 340K
P = (0.269mol . 0.082 L.atm/mol.K . 340K) / 5.38 L
P = 1.39 atm
Now we have the total pressure, we can apply molar fraction so we can know the partial pressure of Kr.
Kr pressure / Total Pressure = Kr moles / Total moles
Kr pressure / 1.39 atm = 0.115 moles / 0.269 moles
Kr pressure = (0.115 moles / 0.269 moles) / 1.39atm
Kr pressure = 0.59 atm
