# Problem: The "fizz" in a carbonated beverage is from carbon dioxide that has been dissolved in the aqueous solution. This is typically achieved by pressuring the "head space" (the empty space above the liquid in the bottle) with carbon dioxide gas.  a. What is the concentration of CO 2 in a soda that has been pressurized with 3.0 atm of CO 2 (in molarity)? Assume a Henry's law constant of 0.0769 M/atm.          b. How does the solubility of CO 2 in water change after it is opened and is at equilibrium with the air (i.e. does it become more or less soluble)?

###### Problem Details

The "fizz" in a carbonated beverage is from carbon dioxide that has been dissolved in the aqueous solution. This is typically achieved by pressuring the "head space" (the empty space above the liquid in the bottle) with carbon dioxide gas.

a. What is the concentration of CO 2 in a soda that has been pressurized with 3.0 atm of CO 2 (in molarity)? Assume a Henry's law constant of 0.0769 M/atm.

b. How does the solubility of CO 2 in water change after it is opened and is at equilibrium with the air (i.e. does it become more or less soluble)?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Henry's Law concept. You can view video lessons to learn Henry's Law. Or if you need more Henry's Law practice, you can also practice Henry's Law practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofThe "fizz" in a carbonated beverage is from carbon dioxide t...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 3 minutes and 22 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Gerhard's class at UNCG.