If CO 2 gas having a partial pressure of 1.67 bar is bubbled through 1 L water at 298 K, the amount of CO 2 dissolved in water in g L -1 is approximately. (Henry's law constant of CO 2 is 1.67 k bar at 298 K )

Question

If CO 2 gas having a partial pressure of 1.67 bar is bubbled through 1 L water at 298 K, the amount of CO 2 dissolved in water in g L -1 is approximately. (Henry's law constant of CO 2 is 1.67 k bar at 298 K ) (A) 24.42 (B) 12.21 (C) 2.44 (D) 1.22

Tardigrade Admin · Accepted Answer

Let pA be the partial pressure of CO 2 and chiA be its mole pA =K H chiA (Henry's law) 1.67 bar =1.67 k bar × chiA (where, xA =0.001) or (nA/nB)=0.001 [∵ Number of moles of water =55 ] nA =0.001 × 55.55 nA =0.056 n=( text Given mass(m)/ text Molecular mass (M))=0.056 ∴ m=0.056 × 44=2.44 g Thus, 2.44 g of CO 2 is dissolved in 1 L water at 298 K

Q. If CO2​ gas having a partial pressure of 1.67 bar is bubbled through 1L water at 298K, the amount of CO2​ dissolved in water in gL−1 is approximately. (Henry's law constant of CO2​ is 1.67k bar at 298K )

24.42

12.21

2.44

1.22

Q. If $C O_{2}$ gas having a partial pressure of $1.67$ bar is bubbled through $1 L$ water at $298 K$ , the amount of $C O_{2}$ dissolved in water in $g L^{- 1}$ is approximately. (Henry's law constant of $C O_{2}$ is $1.67 k$ bar at $298 K$ )