Ok, UMMMM I thought I was good.. Till now..
Ok, 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
Part B: Limiting Reactants
Plastic Cup C
7. Determine which reactant is the limiting reactant in the plastic cup C. Describe your reasoning.
You know I know how to calculate the TY and AY and %Y now, but I'm confused on the finding limiting reactant? umm Let me see if I can figure it out and you let me know if I'm on the right track...
2.02g NaHCO3 mols = 2.02/84 = 0.0240 mols
the ratio is 3/1 for NaHCO3toH3C6H5O7 so do I do 0.0240/3 = citric acid? 0.008 moles citric acid? so since citric acid is smaller but it requires 3 of sodium bicarbonate, would that be the limiting reactant? because it takes more of them? am I figuring this out right?
8. Calculate the theoretical yield of carbon dioxide in the plastic cup C.
2.02/84=0.0240 *44 = 1.056 TY??
9. Calculate the percentage yield in the plastic cup C.
AY = 0.30/1.056 TY = 0.284*100 = 28.4% ?? is this right?
You know I know how to calculate the TY and AY and %Y now, but I'm confused on the finding limiting reactant? umm Let me see if I can figure it out and you let me know if I'm on the right track...
2.02g NaHCO3 mols = 2.02/84 = 0.0240 mols
the ratio is 3/1 for NaHCO3toH3C6H5O7 so do I do 0.0240/3 = citric acid? 0.008 moles citric acid? so since citric acid is smaller but it requires 3 of sodium bicarbonate, would that be the limiting reactant? because it takes more of them? am I figuring this out right?
I can't tell which you're calling the LR. Citric acid is the LR. Based on you 2.02 g it requires 0.008 mols citric acid and you have only 0.004 so you don't have enough citric acid and that makes it the LR.
8. Calculate the theoretical yield of carbon dioxide in the plastic cup C.
2.02/84=0.0240 *44 = 1.056 TY??
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.
9. Calculate the percentage yield in the plastic cup C.
AY = 0.30/1.056 TY = 0.284*100 = 28.4% ?? is this right?
TY needs to be recalculated.
Let me help you understand how to determine the limiting reactant and calculate the theoretical yield and percentage yield.
In order to determine the limiting reactant, you need to compare the moles of each reactant to their stoichiometric coefficients in the balanced equation.
For Cup C, you correctly calculated the moles of sodium bicarbonate (NaHCO3) using its mass of 2.02g and molar mass of 84g/mol: 2.02g / 84g/mol = 0.0240 mol NaHCO3.
The balanced equation shows a ratio of 3 moles of NaHCO3 to 1 mole of citric acid (H3C6H5O7). So, to find the moles of citric acid, you divide the moles of NaHCO3 by 3: 0.0240 mol NaHCO3 / 3 = 0.008 mol citric acid.
From your calculations, you correctly determined that the moles of citric acid (0.008 mol) are smaller than the moles of sodium bicarbonate (0.0240 mol). Since the reaction requires 3 moles of sodium bicarbonate for every mole of citric acid, the citric acid is the limiting reactant. Therefore, your reasoning is correct.
Moving on to the theoretical yield of carbon dioxide (CO2) in Cup C, you can refer to the balanced equation to determine the stoichiometric ratio between citric acid and CO2. The balanced equation shows that 1 mole of citric acid produces 3 moles of CO2.
You calculated the moles of citric acid (0.008 mol), so you can multiply it by the stoichiometric ratio to find the theoretical yield: 0.008 mol citric acid * 3 mol CO2 / 1 mol citric acid = 0.024 mol CO2.
Next, to calculate the percentage yield, you need to compare the actual yield (0.30g CO2) to the theoretical yield (0.024 mol CO2).
First, convert the theoretical yield from moles to grams using the molar mass of CO2 (44 g/mol): 0.024 mol CO2 * 44 g/mol = 1.056g CO2.
Now, you can calculate the percentage yield by dividing the actual yield (0.30g CO2) by the theoretical yield (1.056g CO2) and multiplying by 100: (0.30g CO2 / 1.056g CO2) * 100 = 28.4%.
So, your calculated values for the theoretical yield (TY) and percentage yield (AY) are correct.