Respuesta :
The question is incomplete, here is the complete question:
At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.
Answer: The mass of carbon dioxide that can be dissolved is 1.7 grams
Explanation:
To calculate the molar solubility, we use the equation given by Henry's law, which is:
[tex]C_{CO_2}=K_H\times p_{CO_2}[/tex]
where,
[tex]K_H[/tex] = Henry's constant = [tex]0.031M/atm[/tex]
[tex]C_{CO_2}[/tex] = molar solubility of carbon dioxide gas
[tex]p_{CO_2}[/tex] = partial pressure of carbon dioxide gas = 2.92 atm
Putting values in above equation, we get:
[tex]C_{CO_2}=0.031M/atm\times 2.92 atm\\\\C_{CO_2}=0.0905M[/tex]
To calculate the mass of solute, we use the equation used to calculate the molarity of solution:
[tex]\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}[/tex]
Given mass of carbon dioxide = ? g
Molar mass of carbon dioxide = 44 g/mol
Molarity of solution = [tex]0.0905mol/L[/tex]
Volume of solution = 425 mL
Putting values in above equation, we get:
[tex]0.0905mol/L=\frac{\text{Mass of carbon dioxide}\times 1000}{44g/mol\times 425}\\\\\text{Mass of solute}=\frac{44\times 425\times 0.0905}{1000}=1.7g[/tex]
Hence, the mass of carbon dioxide that can be dissolved is 1.7 grams
