What are the partial pressures and the total pressure in a 2.50 L vessel containing the following mixture of gases at 17.8°C: 0.0274 mol #He#, 0.0431 mol #H_2#, and 0.169 mol #Ne#?

1 Answer
Nov 15, 2015

Answer:

Dalton's law of partial pressure holds that in a gaseous mixture, the pressure exerted by the component is the pressure it would exert if it solely occupied the volume. The total pressure is the sum of the partial pressures.

Explanation:

From the ideal gas equation:

#P=(nRT)/V=(0.2395*molxx0.0821*L*atm*K^(-1)*mol^-1xx290.8K)/(2.50*L)#

I have summed the individual molar quantities to give a total number of moles of gas, as Dalton's law allows me to do. I will get an answer in atmospheres (this is the only unit that will NOT cancel!).