We have `N_2` and `O_2` in the gas mixture. Mole fraction of `N_2` is 0.7

`X_(N_2) = 0.7`

Since mole fraction of both gasses add up to 1;

`X_(O_2) = 1-0.7 = 0.3`

Total pressure `(P_T) = 1.42atm`

Partial pressure = (mole fraction)`xx` (total pressure)

`P_(O_2) = X_(O_2)xxP_T`

...

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We have `N_2` and `O_2` in the gas mixture. Mole fraction of `N_2` is 0.7

`X_(N_2) = 0.7`

Since mole fraction of both gasses add up to 1;

`X_(O_2) = 1-0.7 = 0.3`

Total pressure `(P_T) = 1.42atm`

Partial pressure = (mole fraction)`xx` (total pressure)

`P_(O_2) = X_(O_2)xxP_T`

`P_(O_2) = 0.3xx1.42 = 0.426atm`

** So the partial pressure of `O_2` is 0.426atm**.

*Assumption*

*Both gasses act as ideal gasses.*