# What is the total pressure exerted by a mass of 2.27*g of oxygen gas, and a mass of 0.636*g of helium gas, if the container had a volume of 6.26*L, and the gases were at a temperature of 51 ""^@C?

May 25, 2016

Dalton's Law of Partial Pressures states that the pressure exerted by a component in a gaseous mixture, is precisely the same as it would exert if it ALONE occupied the container,

#### Explanation:

The total pressure is the sum of the individual partial pressures.

From the above:

${P}_{\text{Total" = P_"oxygen" + P_"helium}}$

$=$ $\frac{R \cdot T \cdot {n}_{\text{oxygen")/V+(R*T*n_"helium}}}{V}$

$=$ $\frac{R T}{V} \left\{{n}_{\text{oxygen" + n_"helium}}\right\}$

$=$ $\frac{R T}{V} \left\{\frac{2.27 \cdot g}{32.0 \cdot g \cdot m o {l}^{-} 1} + \frac{0.636 \cdot g}{4.0 \cdot g \cdot m o {l}^{-} 1}\right\}$

R=0.0821*L*atm*K^-1*mol^-1; T=326K; V=6.26L