Answer:
The partial pressure of carbon dioxide in the flask is 0,69 atm and the total pressure in the flask is 1,62 atm
Explanation:
Let think the Ideal gas equation
Pressure . volume = n.R.T
where R = 0,082 L.atm/ mol.K
T is temperature in K (T in °C + 273)
n = moles
In a mixture you have to think P as Total Pressure and n, the total moles (mol from any gas in the mixture)
You have mass, so let's get the moles
H2 = 0,545g/ 2,016 g/m = 0,270 moles
CO2 = 8,89 g/44 g/m = 0,202 moles
Total moles = 0,270 + 0,202 = 0,472 moles
Pressure = (0,472 moles . 0,082L.atm/mol.K . 347K) / 8,30L
Pressure = 1,62 atm
Pressure of CO2 must be calculated by the same rule, just take account moles from CO2
Pressure = (0,202 moles . 0,082L.atm/mol.K . 347K) / 8,30L
Pressure = 0,692 atm
There is another way to solve the partial pressure which involves the molar fraction.
Pressure in one gas / Total pressure = n moles in one gas / Total moles
Pressure CO2 / Total pressure = n moles CO2 / Total moles
Pressure CO2 = (n moles CO2/Total moles). Total pressure
Pressure CO2 = (0,202 moles / 0,472 moles). 1,62 atm
Pressure CO2 = 0,69 atm
