The partial pressure of carbon dioxide in a gas mixture is 3.5 atm. What will be the solubility (in M) of carbon dioxide gas when Henry's Law constant for carbon dioxide is 3.4 x 10-2M/atm

The solubility of carbon dioxide gas is 0.119 M

Explanation:

To calculate the molar solubility, we use the equation given by Henry's law, which is:

where,

= Henry's constant =

= partial pressure of carbon dioxide gas = 3.5 atm

Putting values in above equation, we get:

Hence, the solubility of carbon dioxide gas is 0.119 M

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"