9. Suppose two gases in a container have a total pressure of 1.20 atm. What is the pressure of gas B if the partial pressure of gas A is 0.75 atm?

Md Ariful Islam

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Md Ariful Islam

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Dalton's Law of holds that in a gaseous mixture, the pressure 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 partial pressure.

i.e. $P_"Total"=P_1+P_2+P_3.........$

And here $P_"Total"=1.20*atm=P_A+P_B=0.75*atm+P_B$,

i.e. $P_B=1.20*atm-0.75*atm=??*atm.$

Note that we can use this law to access the number of moles of each gas, given that $P=(nRT)/V$,

i.e. $P_"Total"=(RT)/V{n_1+n_2+...........n_n}$, where $n_i$ is the number of moles of gas $i$.

And we can show that:

$P_i/P_"Total"=n_i/n_"Total"$,

i.e. partial pressure is equivalent to mole fraction.

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