A gaseous mixture was prepared by taking equal mole of CO and N2 .if the total pressure of the mixture was found 1 atmosphere ,the partial pressure of nitrogen (N2) in the mixture is.
Another way. My suspicion is that your chem prof wanted you to get practice on mole fractions.
Assume any number of mols; i.e., 1 is a good number but any number will work.
n CO = 1
n N2 = 1
Total mols = 2
XCO = mols fraction = n CO/total mols = 1/2
XN2 = n N2/total mols = 1/2
pCO = XCO*Ptotal = 1/2 x 1 = 1/2
pN2 = XN2*Ptotal = 1/2 x 1 = 1/2
P V = n R T
V same
n same
R same
T same
so partial pressure of each is 1/2 atm.
To find the partial pressure of nitrogen (N2) in the mixture, we can use Dalton's Law of partial pressures. According to Dalton's Law, the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.
In this case, we know that the total pressure of the mixture is 1 atmosphere. Since equal moles of CO and N2 are taken, the mole fraction of each gas is 1/2. Assuming ideal gas behavior, the partial pressure of N2 can be calculated as:
Partial pressure of N2 = Total pressure * Mole fraction of N2
Therefore, the partial pressure of N2 in the mixture is:
Partial pressure of N2 = 1 atm * (1/2)
= 0.5 atm
So, the partial pressure of nitrogen (N2) in the mixture is 0.5 atmospheres.