The following question is due to a reaction in organic chemistry ethanol from sucrose. I did not properly state in my last post where the reaction came from. I apologize for this (Dr.Bob). I repost the same question: Calculate how many milliliters of carbon dioxide would be produced theoretically from 20g of sucrose of 25 degree Celsius and 1 atmosphere pressure.
The organic reaction is this:
Na3PO4(enzyme)
C12H22O11 + H2O ---> 4CH3CH2OH + 4CO2
I know that 1 mole sucrose yields 4 moles CO2. How can I use the PV=nRT to solve this problem?
(1atm)(V)= (n?)(R constant?)(25C)
Do I need to convert anythings. Please guide me with steps.
P.S. Also, I've never heard of acetaldehyde before. I did a search on it, however it does not help me figure out how its impurity arise in the fermentation of ethanol from sucrose.
The following question is due to a reaction in organic chemistry ethanol from sucrose. I did not properly state in my last post where the reaction came from. I apologize for this (Dr.Bob). I repost the same question: Calculate how many milliliters of carbon dioxide would be produced theoretically from 20g of sucrose of 25 degree Celsius and 1 atmosphere pressure.
The organic reaction is this:
Na3PO4(enzyme)
C12H22O11 + H2O ---> 4CH3CH2OH + 4CO2
Thanks for clearing up the reaction step. The procedure will be the same as I outlined when I wrote a different equation for you. Of course the numbers will change.
Convert 20 g sucrose to mols.
20/molar mass sucrose = ??
Now convert mols sucrose to mols CO2. Use the coefficients in the balanced equation you supplied.
??mols sucrose x (4 mols CO2/1 mol sucrose) = xx mols CO2.
Now you are ready for PV = nRT.
You know P = 1 atm
You solve for V (in liters, then convert that to milliliters).
n = mols CO2 from above.
R = 0.08206 L*atm/mol*K
T = 25 C but convert that to K.
Post your work if you need further assistance. I don't remember a question about acetaldehyde; if there is a question, please repost with it.
Dr. Bob, since I had organic lab at 12:30 today, I missed your response and figured it out while I awaited my data for extraction lab. (I know I should have been better prepared)
So I was able to solve the problem or at least I understood what was happening. I made a mistake in the R constant (I put .82 as opposed to .082) So my answer is wrong overall, but I hope that my steps will enable my teacher to see that I knew what I was doing.
The reason I got stuck earlier was because I did not convert moles sucrose (C12H22O11) in to CO2. But then I realized the question asked for the volume of carbon dioxide and realized that there was a ration of 1:4. From there I understood it. Thx again for your help! Very informative, nonetheless. Perhaps, someone here will benefit. Thx again!
what about the Q. acetaldehyde impurity arise fermentation? Dr. Bob
wel i just wanted to know the final answer or at least the equation. Here is my work
V= (.234)(.082)(298)/760
I'm glad to hear that you were able to figure out the problem on your own and understand the steps involved. It's important to double-check your calculations, especially when it comes to constants like the ideal gas constant (R). I apologize for not catching that error in my previous response.
To recap the steps you took:
1. Convert the mass of sucrose to moles:
20g sucrose / molar mass of sucrose = ??? moles of sucrose
2. Use the stoichiometry of the balanced equation to convert moles of sucrose to moles of CO2:
?? moles sucrose x (4 moles CO2/1 mole sucrose) = ??? moles CO2
3. Now, you can use the ideal gas law equation PV = nRT to calculate the volume of CO2. Rearranging the equation to solve for volume (V), you have:
PV = nRT
V = (nRT)/P
Let's plug in the values:
P = 1 atm
n = ??? moles CO2 (from step 2)
R = 0.08206 L*atm/mol*K (the correct value for the ideal gas constant)
T = 25°C + 273.15 K (convert temperature to Kelvin)
4. Calculate the volume of CO2 in liters:
V = (nRT)/P
5. Convert the volume from liters to milliliters:
1 liter = 1000 milliliters
Make sure to review your calculations and check if the units are consistent throughout the problem. Double-checking your work can help ensure that your final answer is correct. Keep up the good work!