For Cup C
Mass of cup,water,stirrer: 55.15
Mass of sodium bicarbonate: 2.02g
mass of citric acid: 0.77g
total mass: 57.94g
mass of cup,solution, stirrer after reaction: 57.64
difference (CO2): 0.30g
Calculate the theoretical yield of carbon dioxide in the plastic cup C.
** u said**If citric acid is the LR then you should use it to determine the theoretical yield. This calls into question some of the earlier answers since I didn't check them for the LR bit. But it stands to reason that if 1 g NaHCO3 is equivalent to 0.76 g citric acid then if you start with 2.02 g NaHCO3 it will take more than 0.76 g citric acid and there isn't enough there to do anything except with 1g NaHCO3.
So I should be saying 0.008/84 *44? = 0.42% or am I to use the citric acid mass of 192.1? 0.008/192.1 = 0.00042 * 44 ==0.0018 I'm even more confused now... And before I didn't have to calculate the limiting reagent it's just now asking me to.. I don't know.. ughhhhhh..
I don't know why the delay in discussing/asking questions about limiting reagents but then I'm not teaching the course.
To recap, I think you had 2.02g NaHCO3 and 0.77 g citric acid (or was that 0.76 g). To determine the LR reagent and the theoretical yield, I do these the long way.
question 1. How much CO2 can be produced if we used ALL of the NaHCO3 and had all of the citric acid needed.
(2.02/84) x (3 mol CO2/3 mol NaHCO3) x (44 g CO2/1 mol CO2) = about 1.06g CO2
question 2. How much CO2 can be produced if we used ALL of the citric acid and had all of the NaHCO3 needed?
(0.77/192.1) x (3 mol CO2/1 mol citric acid) x (44 g CO2/1 mol CO2) = about 0.53g.
In limiting reagent problems the SMALLER amount always wins because you can't produce more than the limiting reagent will allow. So you will produce about 0.53 g CO2, all of the citric acid is used, some of the NaHCO3 is used and there is some unused. I hope I don't have the numberrs mixed up. I'm trying to do this from memory. (Note: the reason I like to do these LR problems the long way is because when I finish I have the answer to two questions; i.e., 1 is which is the limiting reagent and 2 is how much CO2 was produced and I get that number for calculating theoretical yield. So it may be the long way for some people but I get the complete answer instead of having to work two separate problems of one for the LR part and one for the TY part.
I mention the getting numbers confused because I see your 0.008/192.1 = 0.00042 and I don't know where that came from. Perhaps I do have my numbers mixed up.
To calculate the theoretical yield of carbon dioxide in the plastic cup C, you need to determine the limiting reagent (LR) between sodium bicarbonate (NaHCO3) and citric acid (C6H8O7). The LR is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
1. Calculate the moles of NaHCO3 and C6H8O7 present in the reaction:
Moles of NaHCO3 = mass of NaHCO3 / molar mass of NaHCO3
= 2.02 g / 84.01 g/mol
Moles of C6H8O7 = mass of C6H8O7 / molar mass of C6H8O7
= 0.77 g / 192.13 g/mol
2. Calculate the ratio of moles between NaHCO3 and C6H8O7:
Ratio = Moles of C6H8O7 / Moles of NaHCO3
3. Compare the ratios:
If the ratio is less than 1, it means that NaHCO3 is the LR.
If the ratio is greater than 1, it means that C6H8O7 is the LR.
In this case, based on the given information, it seems that citric acid (C6H8O7) is the limiting reagent for the reaction since there is not enough citric acid to react with the given amount of NaHCO3.
Now, to calculate the theoretical yield of carbon dioxide (CO2):
4. Calculate the moles of CO2 produced from the LR (C6H8O7):
Moles of CO2 = Moles of C6H8O7 * (2 moles of CO2 / 1 mole of C6H8O7)
5. Calculate the mass of CO2 produced:
Mass of CO2 = Moles of CO2 * molar mass of CO2
Finally, to calculate the percentage yield of CO2, you need the actual yield of CO2. The given information indicates that the difference (CO2) is 0.30g, so you can use that as the actual yield.
6. Calculate the percentage yield of CO2:
Percentage Yield = (Actual yield / Theoretical yield) * 100
Plug in the values into the equations to get the final answer.