Respuesta :
Answer: The concentration of nitrogen gas when the partial pressure is 1.086 atm above water is [tex]6.62\times 10^{-4}mol/L[/tex]
Explanation:
To calculate the molar solubility, we use the equation given by Henry's law, which is:
[tex]C_{N_2}=K_H\times p_{N_2}[/tex]
where,
[tex]K_H[/tex] = Henry's constant = ?
[tex]C_{N_2}[/tex] = molar solubility of nitrogen gas = [tex]4.52\times 10^{-4}mol/L[/tex]
[tex]p_{N_2}[/tex] = partial pressure of nitrogen gas = 0.741 atm
Putting values in above equation, we get:
[tex]4.52\times 10^{-4}mol/L=K_H\times 0.741atm\\\\K_H=\frac{4.52\times 10^{-4}mol/L}{0.741atm}=6.10\times 10^{-4}mol/L.atm[/tex]
Now, calculating the concentration when pressure is changed by using above equation:
[tex]p_{N_2}[/tex] = 1.086 atm
[tex]K_H=6.10\times 10^{-4}mol/L.atm[/tex]
Putting values in above equation, we get:
[tex]C_{N_2}=6.10\times 10^{-4}mol/L.atm\times 1.086atm\\\\C_{N_2}=6.62\times 10^{-4}mol/L[/tex]
Hence, the concentration of nitrogen gas when the partial pressure is 1.086 atm above water is [tex]6.62\times 10^{-4}mol/L[/tex]
