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The solubility of CO2 in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility under atmospheric conditions? (The partial pressure of CO2 in air is 0.0003 atm.) Assume that CO2 obeys Henry’s law.

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Willchemistry

Hey there!:

Henry law solubility proportional to partial pressure of gas over a solvent  :

for pressure of 1 atm s = 0.034

fro partial pressure of =0 .0003

Therefore :

Solubility = 0.0003 / 1 * 0.034

Solubility = 1.02 * 10⁻⁵ mol/L

Hope this helps!

okpalawalter8

Answer:

  • Its solubility under atmospheric conditions = [tex]1.02*10^{-5} mol/L[/tex]

Explanation:

From Henry's law

c = kP

where

c = molar concentration

k = proportionality constant

P = pressure

Hence, solubility in water

[tex]k = \frac{c}{P}\\\\k = \frac{0.34}{1}\\\\k = 0.034mol/L-atm[/tex]

The solubility of [tex]CO_2[/tex] under atmospheric conditions in air is

[tex]c = kP\\\\c = 0.034 * 0.0003\\\\c = 1.02*10^{-5} mol/L[/tex]

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