Question

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?

Answer 1

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.