I am stuggling with my chemistry experiment.
I am given thr following:
The reaction of citric acid and sodium bicarbonate is written as
H3C6H5O7(aq) + 3NaHCO3(aq) --> Na3C6H5O7(aq) + 3H2O(l) + 3CO2(g)
1.) Mass of cup A, water, and stirrer = 54.3 g
2.) Mass of sodium bicarbonate = 1.00g
3.) Mass of citric acid = .76g
4.) Total Mass = 56.06g
5.) Total Mass after reaction= 55.63g
6.) Differnece 0.43g
I'm asked to calculate the theoretical yield of carbon dioxide from 1.00g of sodium bicarbonate. And to calculate the precentage yield in the plastic cup A.
I am totally lost and don't know how to even begin to set up equations to solve. Any help appreciated.
Several problems, including a limiting reagent problem, all rolled into one.
mol NaHCO3 = grams/molar mass = ?
mols citric acid = g/molar mass = ?
Convert mols NaHCO3 to mols CO2 using the coefficients in the balanced equation.
That's ?mol NaHCO3 x (3 mols CO2/3 mols NaHCO3) = ? mol NaHCO3 x 1/1 = ?mol CO2.
Do the same with citric acid.
? mols citric acid x (3 mols CO2/1 mol H3C6H5O7) = ?mols citric acid x 3 = ?
It is likely that these two values for mols CO2 will not agree which means one of them is wrong. The correct value in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent. Then smaller value mols CO2 x molar mass CO2 = grams CO2. This is theoretical yield (TY).
The actual yield (AY) in the problem is 0.43 g CO2.
%yield = (AY/TY)*100 = ?
Am I doing this right?
mol NaHCO3 = grams/molar mass = 1/85 = 0.0117647059*3=0.0352941176
mols citric acid = g/molar mass = 1/316 = .003164557*3=0.009493671
So, the second one is correct and is the limiting reactant.
0.009493671 mols CO2 x 44 CO2 = 0.417721524 = .42 grams CO2. This is theoretical yield (TY).
The actual yield (AY) in the problem is 0.43 g CO2.
%yield = (0.43/0.42)*100 = 102.3809524 = 102%
is any of this right?
The procedure is right because you're following my directions; however, your numbers are wrong.
1. The molar mass NaHCO3 is not 85.
2. The molar mass citric acid is not 316.
3. The mass citric acid is not 1 g (from the problem.
To calculate the theoretical yield of carbon dioxide (CO2), we need to determine the stoichiometry of the reaction. The balanced equation you provided is:
H3C6H5O7(aq) + 3NaHCO3(aq) → Na3C6H5O7(aq) + 3H2O(l) + 3CO2(g)
From the equation, we can see that 1 mole of citric acid (C6H8O7) reacts with 3 moles of sodium bicarbonate (NaHCO3) to produce 3 moles of carbon dioxide gas (CO2).
To start, we need to convert the mass of sodium bicarbonate (NaHCO3) provided (1.00g) into moles. The molar mass of sodium bicarbonate is:
NaHCO3: (1 x 22.99g/mol) + (1 x 1.01g/mol) + (3 x 16.00g/mol) = 84.01 g/mol
Using this molar mass, we can calculate the number of moles of sodium bicarbonate:
Number of moles of NaHCO3 = Mass of NaHCO3 (in grams) / Molar mass of NaHCO3
Number of moles of NaHCO3 = 1.00g / 84.01g/mol
Next, we use the stoichiometry of the reaction to determine the theoretical yield of carbon dioxide (CO2). Since we know that 1 mole of sodium bicarbonate produces 3 moles of carbon dioxide, we can set up the following ratio:
(3 mol CO2 / 1 mol NaHCO3) x (number of moles of NaHCO3)
The moles of NaHCO3 cancel out, leaving us with the number of moles of carbon dioxide:
Number of moles of CO2 = (3 mol CO2 / 1 mol NaHCO3) x (number of moles of NaHCO3)
Once we have the number of moles of carbon dioxide, we can convert it to grams if necessary using the molar mass of carbon dioxide (CO2).
To calculate the percentage yield, we need to compare the actual yield with the theoretical yield. The actual yield is given as the difference in mass before and after the reaction (0.43g). The percentage yield is calculated as follows:
Percentage yield = (Actual yield / Theoretical yield) x 100
Substituting the values we have, you can calculate the theoretical yield and the percentage yield of carbon dioxide for your experiment.
I hope this explanation helps you understand how to approach this problem in the future!