Answer: The partial pressure of nitrogen is 1.25 atm
Explanation:
From ideal gas equation:
[tex]PV=nRT[/tex]
where,
R = Gas constant = [tex]0.0821\text{ L atm }mol^{-1}K^{-1}[/tex]
T = temperature of the gas = 273K (at STP)
P = pressure of the gas = 1 atm (at STP)
n = number of moles = 0.1 +0.4 = 0.5
To calculate the partial pressure of the solution, we use the law given by Dalton, which is:
[tex]P_T=\sum_{i=1}^n (p_i\times \chi_i)[/tex]
Or,
[tex]P_T=[(p_{\text{N_2}}\times \chi_{N_2})[/tex]
where, [tex]\chi_{N_2})[/tex]= mole fraction nitrogen =[tex]\frac{\text {moles of nitrogen}}{\text {total moles}}=\frac{0.4}{0.5}=0.8[/tex]
We are given:
Total pressure = 1 atm
Putting values in above equation, we get:
[tex]1=0.8\times p_{N_2}[/tex]
[tex]p_{N_2}=1.25atm[/tex]
Thus the partial pressure of nitrogen is 1.25 atm
