A tank contains a mixture of 52.5g of oxygen and 65.1 g of `CO_(2)` at 300 K the total pressure in the tanks is 9.21 atm. Calculate the partial pressure (in atm). Of each gas in the mixture.

Explanation

`m_(O_(2))=52.5gP_(O_(2))=?`
`m_(CO_(2))=65.1gP_(CO_(2))=?`
`T=300KP=9.21atm`
`P_(O_(2))=X_(O_(2))xx` Total Pressure
`X_(O_(2))=(n_(O_(2)))/(n_(O_(2))+n_(CO_(2)))`
`n_(O_(2))=("Mass of"O_(2))/("Molar mass of "O_(2))`
`=(52.5g)/(32gmol^(-1))=1.64mol`
`n_(CO_(2))=("Mass of "O_(2))/("Molar mass of "CO_(2))`
`(65.1g)/(44gmol^(-1))=1.48mol`
`X_(O_(2))=(n_(CO_(2)))/(n_(O_(2))+n_(CO_(2)))=(1.64)/(3.12)=0.53`
`X_(CO_(2))=(n_(CO_(2)))/(n_(O_(2))+n_(CO_(2)))=(1.48)/(3.12)=0.47`
`P_(O_(2))=X_(O_(2))xx` Total pressure
`0.53xx9.21` atm =4.88 atm
`P_(CO_(2))=X_(CO_(2))xx` Total pressure
`=0.47xx9.21` atm =4.33 atm.