Answer:
Partial pressure = 4689 torr
Explanation:
Given:
Concentration of CO2, c = 0.21 M= 0.21 mol/L
Henry's constant, k for CO2 = 3.4*10^-2 mol/L-atm
To determine:
the partial pressure, P
Calculation:
As per Henry's law, the concentration c of a gas is related to the pressure, p as follows:
[tex]C = k*p\\\\p = \frac{C}{k} = \frac{0.21 mol/L}{3.4*10^{-2}mol/L-atm} =6.17 atm[/tex]
Conversion from atm to torr
1 atm = 760 torr
[tex]p =6.17*760 = 4689 torr[/tex]
