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
May 25, 2016

Answer:

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#