Following data has been given for CO2 for the concentration in H2O Temperature Henry’s constant Pressure 273 K 600 atm 0.30 atm 333 K 3400 atm P2 If solution of CO2 in H2O is heated from 273 to 333 K pressure (P2) needed to keep CO2 in the solution is

Question

Following data has been given for CO2 for the concentration in H2O Temperature Henry’s constant Pressure 273 K 600 atm 0.30 atm 333 K 3400 atm P2 If solution of CO2 in H2O is heated from 273 to 333 K pressure (P2) needed to keep CO2 in the solution is (A) 0.108 atm (B) 1.7 atm (C) 0.212 atm (D) 0.468 atm

Tardigrade Admin · Accepted Answer

By Henryâs law at 273 K, chico2 (mole fraction of CO2) =(P/KH)=(0.30/600) By Henryâs law at 333 K, chico2=-(P/KH)=(P2/3400) ∴ (p2/3400)=(0.30/600) P2=(0.30×3400/600)=1.7 atm

Q. Following data has been given for CO2​ for the concentration in H2​O Temperature Henry’s constant Pressure 273 K 600 atm 0.30 atm 333 K 3400 atm P2​ If solution of CO2​ in H2​O is heated from 273 to 333K pressure (P2​) needed to keep CO2​ in the solution is

0.108 atm

1.7 atm

0.212 atm

0.468 atm

By Henry’s law at 273 K, χco2​​ (mole fraction of CO2​) =KH​P​=6000.30​ By Henry’s law at 333K, χco2​​=−KH​P​=3400P2​​ ∴3400p2​​=6000.30​ P2​=6000.30×3400​=1.7atm

By Henry’s law at 273 K,
$χ_{c o_{2}}$ (mole fraction of $C O_{2})$ $= \frac{P}{K _{H}} = \frac{0.30}{600}$
By Henry’s law at $333 K$ ,
$χ_{c o_{2}} = - \frac{P}{K _{H}} = \frac{P _{2}}{3400}$
$∴ \frac{p _{2}}{3400} = \frac{0.30}{600}$
$P_{2} = \frac{0.30 \times 3400}{600} = 1.7 a t m$