# Mixture containing .538mol He gas, .315mol Ne gas .103 Ar gas, is confined in 7.00-L vessel at 25^oCelsius. How do you calculate partial pressure of each gas in mixture? How would you calculate the total pressure of the mixture?

Feb 23, 2017

$\text{Dalton's law of partial pressures states that.........}$

#### Explanation:

$\text{Dalton's law of partial pressures states that in a gaseous}$
$\text{partial pressure exerted by a component gas is the same as}$
$\text{the pressure it would exert if it alone occupied the container.}$

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

Here ${P}_{\text{Total"=P_"He"+P_"Ne"+P_"Ar}}$

$= \frac{{n}_{\text{He"RT)/V+(n_"Ne"RT)/V+(n_"Ar}} R T}{V}$

$= \frac{R T}{V} \left({n}_{\text{He"+n_"Ne"+n_"Ar}}\right)$

You have the molar quantities; you have the temperature, and volume; you have $R = 0.0821 \cdot L \cdot a t m \cdot {K}^{-} 1 \cdot m o {l}^{-} 1$. Have at it.