[apaturia]

A sodastream container contains water and CO2. The CO2 is at an constant pressure of 2 atm. The molar mass of CO2 is 44 g mol^1-.
Kb at 5 degrees celcius is 15 atm mol^-1 kg. Kb at 30 degrees celcius is 30 atm mol^-1 kg.
1) Calculate for each temperature (5 degrees C and 20 degrees C) how many grams of CO2 is dissolved in 1 liter of water (assume that the density is the same as plain water)
2) A student now drinks 0,33 L of the soda that has been made at 5 degrees celcius. In the mouth and stomach, the soda is now heated to a temperature of 37 degrees celcius at P=1 atm. Assuming that CO2 is an ideal gas, how big a volume of CO2 (in L) has been developed when all the bubbles of CO2 has left soda?

I have no clue how to do this. I tried to calculate the molar fraction of CO2 under both temperatures, but that gives me no number i can use. I don't know the total number of moles in the solution, and therefore I can not calculate the number of moles of CO2 even knowing the fraction of CO2.

THX!!!

[AWK]

http://www.chemicalforums.com/index.php?topic=65859.0

[apaturia]

I've added something to the post.

[AWK]

You should show your attempt.

[Borek]

What is Kb? How is it defined? How is it related to the problem?