Exactly 1.0 mole of oxygen and 7.0 moles of nitrogen gas are in a container. The total gas pressure is 5.7 atm. What is the partial pressure of nitrogen in atm?
I'm not sure how to go about setting up the problem. Any help is appreciated!
mol fraction = X
XO2 = nO2/total mols
XN2 = nN2/total mols
Then pO2 = XO2*Ptotal
and pN2 = XN2*Ptotal
Got it, thanks!
To solve this problem, we need to use the concept of partial pressure. According to Dalton's law of partial pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.
To find the partial pressure of nitrogen gas, we first need to calculate the mole fraction of nitrogen in the mixture. The mole fraction (X) is defined as the ratio of the moles of a specific gas to the total moles of all gases present in the mixture.
In this case, we have 1.0 mole of oxygen and 7.0 moles of nitrogen, so the total moles of gas in the mixture is 1.0 + 7.0 = 8.0 moles.
The mole fraction of nitrogen (X_N2) is given by:
X_N2 = (moles of N2) / (total moles of gas)
= 7.0 moles / 8.0 moles
= 0.875
Now, we can calculate the partial pressure of nitrogen using the equation:
Partial pressure of N2 = Mole fraction of N2 * Total pressure
Partial pressure of N2 = 0.875 * 5.7 atm
= 4.9875 atm
Therefore, the partial pressure of nitrogen gas in the container is approximately 4.99 atm.