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A gaseous mixture was prepared by taking equal moles of CO and $N_2$. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen ($N_2$) in the mixture is
A
1 atm
B
0.5 atm
C
0.8 atm
D
0.9 atm
Detailed Solution
Dalton's law: partial pressure of a gas = mole fraction of the gas × total pressure.
Let the moles of CO = moles of $N_2$ = n.
Mole fraction of $N_2$ = $\frac{n}{n + n} = \frac{1}{2}$
$p_{N_2} = \frac{1}{2}\times1$ atm
$p_{N_2} = 0.5$ atm
Let the moles of CO = moles of $N_2$ = n.
Mole fraction of $N_2$ = $\frac{n}{n + n} = \frac{1}{2}$
$p_{N_2} = \frac{1}{2}\times1$ atm
$p_{N_2} = 0.5$ atm