A 2.0 liter balloon at a temperature of 25°C contains 0.1 mol of oxygen and 0.4 mol of nitrogen, what is the partial pressure of nitrogen?

1 Answer
anor277
Aug 8, 2016

Approx. #5*atm# with respect to #N_2#.

Explanation:

Dalton's law of partial pressures states that in a gaseous mixture, the pressure exerted by a component is the same as the pressure it would exert if it ALONE ooccupied the container. The total pressure, is the sum of the partial pressures.

So given this, I merely have to solve the Ideal Gas equation:

#P_"dinitrogen"=(n_"nitrogen"*R*T)/(V)# #=# #(0.4*cancel(mol)xx0.0821*cancelL*atm*cancel(K^-1)*cancel(mol^-1)xx298*cancelK)/(2*cancelL)#

I get an answer in #atm#, as required.

Related questions
See all questions in Partial Pressure
Impact of this question
5622 views around the world
You can reuse this answer
Creative Commons License