A sealed container comtains 1.50 mol of nitrogen gas, 2.00 mol of oxygen gas and 3.50 mol of argon gas. If the total pressure is 900 kPa, what is the pressure of the nitrogen gas?
I don't know which formula to use
Didn't I do a similar one for you yesterday.
Find total mols gase
Find mole fraction (XN2) of N2.
Then pN2 = XN2*Ptotal.
The problem is i don't understand the mole fraction
mol fraction N2 = mol N2/total mols.
and if you want mol fraction of the others it is
XAr = mols Ar/total mols
XO2 = mols O2/total mols.
To solve this problem, you can use Dalton's law of partial pressures. According to Dalton's law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas.
To find the partial pressure of nitrogen gas, you need to determine its mole fraction in the mixture. The mole fraction is calculated by dividing the number of moles of the nitrogen gas by the total number of moles of all the gases in the container.
Mole fraction of nitrogen gas (X_N2) = Moles of nitrogen gas / Total moles of all gases
X_N2 = 1.50 mol / (1.50 mol + 2.00 mol + 3.50 mol)
= 1.50 mol / 7.00 mol
= 0.214
The mole fraction of oxygen gas can be calculated in a similar manner:
X_O2 = 2.00 mol / (1.50 mol + 2.00 mol + 3.50 mol)
= 2.00 mol / 7.00 mol
= 0.286
Finally, the mole fraction of argon gas can be calculated:
X_Ar = 3.50 mol / (1.50 mol + 2.00 mol + 3.50 mol)
= 3.50 mol / 7.00 mol
= 0.500
Now, you can use the mole fractions to calculate the partial pressure of nitrogen gas. Simply multiply the total pressure by the mole fraction of nitrogen gas:
Partial pressure of nitrogen gas (P_N2) = X_N2 * Total pressure
= 0.214 * 900 kPa
= 192.6 kPa
Therefore, the pressure of the nitrogen gas is approximately 192.6 kPa.