If the partial pressure of CO2 is 2.87 atm the soluability in H2O is known to be 4.68 M. What would be the soluability of CO2 in H2O if the partial pressure is increased to 7.60 atm? Assume the temp is held constant.
would it work to set up a proportion for this question? if not, how should i set it up???
partial pressure CO2 = kc
Knowing p = 2.87 atm when c is 4.68 M allows k to be calculated. Then k and p can be used to calculate the new solubility (note spelling) in mola/L. Post your work if you get stuck.
thank you
Yes, setting up a proportion is a valid approach to solve this problem. Here's how you can set it up:
The solubility of CO2 in water is directly proportional to its partial pressure. Therefore, you can set up the proportion as follows:
(solubility at partial pressure 1) / (partial pressure 1) = (solubility at partial pressure 2) / (partial pressure 2)
Let's plug in the values given in the question.
(solubility at partial pressure 1) / (2.87 atm) = (solubility at partial pressure 2) / (7.60 atm)
Now, you can solve for the solubility at partial pressure 2:
(solubility at partial pressure 2) = (solubility at partial pressure 1) * (partial pressure 2) / (partial pressure 1)
Given that the solubility at partial pressure 1 is 4.68 M, and partial pressure 2 is 7.60 atm, and partial pressure 1 is 2.87 atm, you can substitute these values into the equation:
(solubility at partial pressure 2) = 4.68 M * (7.60 atm) / (2.87 atm)
By evaluating this expression, you will obtain the solubility of CO2 in water when the partial pressure is increased to 7.60 atm, assuming the temperature is held constant.