# A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?

Mar 27, 2017

#### Answer:

P_(H_2)=25%xxP_"Total"=0.31*atm

#### Explanation:

P_"Total"=(n_"Total"RT)/V

$= \frac{{n}_{{H}_{2}} + {n}_{\text{other gases}}}{V}$

But n_(H_2)=25%xxn_"Total".

And thus P_(H_2)=25%xxP_"Total"=25%xx1.24*atm=??

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This treatment relies on $\text{Dalton's Law of Partial Presssures}$, which states that in

$\text{in a gaseous mixture, the partial pressure exerted}$
$\text{by a gaseous component, is the same as the pressure it would}$
$\text{exert if it ALONE occupied the container.}$

$\text{The total Pressure is the sum of the individual partial pressures.}$