##P_”Total”## ##=## ##P_1+P_2+…….P_n##

In a gaseous mixture, the exerted by a component, is the same as the pressure it would exert if it ALONE occupied the container. The total pressure is the sum of the individual pressures. fraction of a component gas is proportional to the partial pressure.

Clearly, the total number of moles of gas is……….

##n_”Total”## ##=## ##n_1+n_2+…….n_n##

And ##P_”Total”=P_1+P_2………+P_n##

But given ideality, then ##P_i=(n_iRT)/V##

So ##P_”Total”## ##=## ##(RT)/V{n_1+n_2+…….n_n}##

And ##P_i## ##=## ##(n_iRT)/V## ##=## ##n_i/(n_1+n_2+…….n_n)xxP_”Total”##

Again, ##P_”Total”## ##=(n_1+n_2+n_3………+n_n)(RT)/V##

It is worthwhile spending a bit of time on the equation, and checking where you use .

##P_”Total”## ##=## ##P_1+P_2+…….P_n##

In a gaseous mixture, the exerted by a component, is the same as the pressure it would exert if it ALONE occupied the container. The total pressure is the sum of the individual pressures. fraction of a component gas is proportional to the partial pressure.

Clearly, the total number of moles of gas is……….

##n_”Total”## ##=## ##n_1+n_2+…….n_n##

And ##P_”Total”=P_1+P_2………+P_n##

But given ideality, then ##P_i=(n_iRT)/V##

So ##P_”Total”## ##=## ##(RT)/V{n_1+n_2+…….n_n}##

And ##P_i## ##=## ##(n_iRT)/V## ##=## ##n_i/(n_1+n_2+…….n_n)xxP_”Total”##

Again, ##P_”Total”## ##=(n_1+n_2+n_3………+n_n)(RT)/V##

It is worthwhile spending a bit of time on the equation, and checking where you use .