You have a sealed 2 liter flask that contains nothing but water and carbon dioxide. The flask is halffilled with liquid water, has a temperature of 25°c, and t
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1. User Answers lhmarianateixeira
In this exercise we want to calculate the amount of moles, so this is going to be:
[tex](4.6)(10^{3}) \ mols \ CO_2[/tex]
Knowing that Henry's law is given by:
[tex]C = KHP[/tex]
Where constants are given by:
 C = Concentration
 KH = Henry's law constant = [tex]0.033 m/atm[/tex]
 P = partial pressure = [tex]0.07 atm[/tex]
Before we can find the concentration of CO2 (and hence the moles of CO2), we first need to find its partial pressure. We look up the vapor pressure of water at 25º and find it to be 0.03 atm. Since the total pressure is equal to 0.1 atm, this mean the partial pressure of:
[tex]CO_2 = 0.1 \ atm  0.03 \ atm = 0.07 \ atm[/tex]
Now using Henry's law, we find the concentration:
[tex]C = (0.033)*( 0.07) = (2.31)*(10^{3})[/tex]
Converting to moles of CO2, we have:
[tex](2.31)*(10^{3})*( 2) = (4.6)*(10^{3})[/tex]
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