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?

1 Answer
anor277
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_"Total" = P_"oxygen" + P_"helium"

= (R*T*n_"oxygen")/V+(R*T*n_"helium")/V

= (RT)/V{n_"oxygen" + n_"helium"}

= (RT)/V{(2.27*g)/(32.0*g*mol^-1)+(0.636*g)/(4.0*g*mol^-1)}

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

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