Question

Suppose that Daniel has a 3.00 L bottle that contains a mixture of O2 , N2 , and CO2 under a total pressure of 5.30 atm. He knows that the mixture contains 0.210 mol N2 and that the partial pressure of CO2 is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O2

Answer 1

`P_(O_2)=3.48atm`

Step-by-step explanation:

Hello.

In this case, we need to use the Dalton's law equation and the ideal gas equation for this mixture containing oxygen, nitrogen and carbon dioxide:

`P_T=P_(O_2)+P_(N_2)+P_(CO_2)`

`PV=nRT`

We know that the partial pressure of carbon dioxide is 0.250 atm and the moles of nitrogen are 0.210 mol, so we can compute its partial pressure via the ideal gas equation:

`P_(N_2)=(n_(N_2)RT)/(V)=(0.21mol*0.082(atm*L)/(mol*K)*273K)/(3.00L)=1.57atm`

Thus the partial pressure of oxygen results:

`P_(O_2)=P_T-P_(N_2)-P_(CO_2)\\\\P_(O_2)=5.30atm-1.57atm-0.250atm\\\\P_(O_2)=3.48atm`

Best regards!