Calculating Volume of CO2 Released from a Can

  • Thread starter rocomath
  • Start date
  • Tags
    Co2 Volume
In summary, the conversation discusses the process of making a soft drink by dissolving CO2 in a flavored solution and sealing it in an aluminum can. The problem is to determine the volume of CO2 released when the can is opened at a lower pressure and all the CO2 escapes. The conversation mentions the use of the Henry law and the ideal gas law to solve the problem.
  • #1
rocomath
1,755
1
I am so lost as to how I should approach this problem

A soft drink is made by dissolving CO2 @ 3.00 atm in a flavored solution and sealing the solution in an aluminum can @ 20C. What volume of CO2 is released when a 355-ml can is opened to 1.00 atm @ 20C and all the CO2 is allowed to escape?

i have the constant for CO2 @ 20C but from there, I'm confused? S(CO2) = k(CO2 @ 20C) x P(CO2)
 
Physics news on Phys.org
  • #2
Since the temperature remains the same at the two temperatures, and the solvent as well, the Henry law constant remains the same for the unopened can and the opened one. The relationship you are looking for is:

C1/P1 = C2/P2

where C1 is the concentration of CO2 at 3 atm. (20C), P1 is 3 atm and P2 is 1 atm.

Be careful regarding the units of k, the Henry constant. It should be in units of atm/C, where 'C' is in the same units as C1 and C2.
 
  • #3
thanks! i was able to do it with a little more thinking.

i had to eventually use the ideal gas law.
 

FAQ: Calculating Volume of CO2 Released from a Can

How do you calculate the volume of CO2 released from a can?

The volume of CO2 released from a can can be calculated by first measuring the can's initial volume and temperature, then recording the change in volume and temperature after the can is opened. The ideal gas law, PV=nRT, can then be used to calculate the number of moles of CO2 released. Finally, using the molar volume of CO2 at the given temperature and pressure, the volume of CO2 released can be calculated.

What is the molar volume of CO2 at different temperatures and pressures?

The molar volume of CO2 varies depending on the temperature and pressure. At standard temperature and pressure (STP), which is 0°C and 1 atmosphere, the molar volume of CO2 is 22.4 liters per mole. However, at higher temperatures and pressures, the molar volume will decrease due to the gas becoming more dense.

How does the volume of CO2 released from a can vary between different types of carbonated beverages?

The volume of CO2 released from a can will vary between different types of carbonated beverages due to the varying levels of carbonation in each beverage. For example, a can of soda will release more CO2 than a can of sparkling water, as soda has a higher level of carbonation. The temperature and pressure of the beverage can also affect the volume of CO2 released.

What factors can affect the accuracy of calculating the volume of CO2 released from a can?

The accuracy of calculating the volume of CO2 released from a can can be affected by several factors. These include variations in temperature and pressure, differences in the level of carbonation in the beverage, and potential errors in measuring the initial and final volumes and temperatures. Additionally, external factors such as shaking the can or pouring it into a glass can also affect the accuracy of the calculation.

Why is it important to calculate the volume of CO2 released from a can?

Calculating the volume of CO2 released from a can is important for several reasons. Firstly, it can provide information about the level of carbonation in the beverage, which can affect its taste and quality. Secondly, it can help with quality control in production processes, ensuring that the correct amount of CO2 is added to the beverage. Additionally, understanding the volume of CO2 released can also have environmental implications, as excess CO2 can contribute to climate change.

Similar threads

How to Calculate Final Pressure in a CO2-Saturated Sealed Vessel?
Replies
4
Views
2K
What Volume of CO2 is Produced from H3PO4 and Na2CO3 Reaction?
Replies
4
Views
3K
Why Does Removing CO2 Make a NaHCO3 Solution More Basic?
Replies
1
Views
6K
CO2 forms from water and antacid tablet
Replies
4
Views
3K
Chemistry Partial pressure and moles problem?
Replies
2
Views
4K
Calculating Pressure Change in Gaseous Reaction: CO2 and BaO
Replies
2
Views
5K
Volume of CO2 from a Tank at 30psi
Replies
8
Views
3K
Calculating Synthesis Gas Volume for Water Heating: A Combustion Problem
Replies
1
Views
3K
Calculating Heat Transfer in a Cylinder with CO2 Gas at Different Temperatures
Replies
3
Views
1K
Gas laws problem (need quick help )
Replies
2
Views
2K

Hot Threads

Recent Insights

Back
Top