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The partial pressure of CO2 gas above the liquid in a carbonated drink is 0.45 atm. Assuming that the Henry's law constant for CO2 in the drink is that same as that in water, 3.7 x 10-2 mol/L atm, calculate the solubility of carbon dioxide in this drink.

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sebassandin

Answer:

[tex]M_{CO_2}=0.01665M[/tex]

Explanation:

Hello,

In this case, the Henry's law allows us to relate the molar concentration and partial pressure of a solute (carbon dioxide) in a solution (solvent is water) by:

[tex]M_{CO_2}=H_{CO_2}p_{CO_2}[/tex]

Whereas we introduce the Henry constant, therefore, we can easily compute the molar solubility by:

[tex]M_{CO_2}=p_{CO_2}*H_{CO_2} =0.45atm*3.7x10^{-2}\frac{M}{atm}\\\\M_{CO_2}=0.01665M[/tex]

Regards.

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