# A mixture of oxygen, hydrogen, and nitrogen exerts a total pressure of 378 kPa. If the partial pressures of oxygen and hydrogen are 212 kPa and 101 kPa respectively, what is the partial pressure exerted by nitrogen?

Sep 10, 2017

${P}_{{N}_{2}} = 65 \cdot k P a \ldots \ldots \ldots . .$

#### Explanation:

Old Dalton's law of partial pressures states that in a gaseous mixture, the partial pressure exerted by a component gas is the same as the pressure it would exert IF IT ALONE occupied the container.....

And thus....${P}_{\text{Total}} = {P}_{{N}_{2}} + {P}_{{O}_{2}} + {P}_{{H}_{2}}$....

i.e. ${P}_{{N}_{2}} =$ ${P}_{\text{Total}} - {P}_{{O}_{2}} - {P}_{{H}_{2}}$

={378-212-101}*kPa=??*kPa