VERMONT TECHNICAL COLLEGE
Chemical Reactions:
Stoichiometry
Lab Report
Taylor Fitzgerald
4/15/2014
CHE1020
Spring 2014
TO: Professor Michelle Sama
FROM: Taylor Fitzgerald, CIT Student
LAB PARTNER: Sam Brissette
DATE: April 15, 2014
SUBJECT: Chemical Reactions - Stoichiometry
Purpose:
The purpose of this lab is to perform the reaction of sodium bicarbonate with
sulfuric acid and see how close the actual product yield comes to the theoretical yield.
Summary:
Successfully balancing the equation, figuring out the theoretical and actual yield,
solving for the percentage, solving the mean, and solving the standard deviation are the
main purpose for this lab. Once each individual grasps the understanding of theoretical
and actual yield, each individual will have a better understanding of the reaction of
sodium bicarbonate with sulfuric acid.
Procedures:
To first start off, each group had to balance out the equation. It was:
2 NaHCO3(s) + 1 H2SO4(aq)  2 CO2(g) + 2 H2O(l) + 1 Na2SO4(aq)
After successfully completing the balanced equation is when each group will start their
labs. This lab will be trailed 3 times.
2. Fill a burette no more than half way with 1 M of sulfuric acid (H2SO4).
3. Get a clean solo cup with a lid.
4. Measure out approximately 0.200 grams of baking soda (NaHCO3) into the solo cup.
5. Using stoichiometry, each group then calculates the mass of CO2 gas. The CO2 was
produced during the reaction above. This number will be the theoretical yield.
6. Before starting the reaction, each group must find the total mass of all the equipment
and reactants. This includes the solo cup with baking soda, the lid, and the burette with
sulfuric acid.
7. Be sure to push the baking soda to one side of the solo cup before starting the reaction
because it will make it react quicker and better later on. Place the lid onto the solo cup
before starting the reaction too. The lid is for the purpose of having the sulfuric acid not
bubble or splatter onto the table and/or an individual’s skin. Inserting the pipette tip
through the hole in the lid and begin adding the sulfuric acid, drop by drop, into the solo
cup. (Don’t count the drops). When there is no more bubbling occurring, the reaction is
then complete.
8. Now that the reaction is complete, open the lid momentarily to allow the CO2 gas to
escape. Now that everything is mellow, record the total mass after the reaction of all the
equipment and left over products.
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CHE1020
Spring 2014
9. Subtract the total mass after the reaction from the total mass before the
reaction to come up with the amount of CO2 gas that was produced and lost in the air.
This is the actual/experimental yield.
10. Rinse and thoroughly dry the solo cup and lid.
11. Repeat all the steps above two more times to make for three trials.
12. Complete all calculations.
Results:
Table 1: Limiting Reagent Amounts
Part A
Mass of NaHCO3
Trial One
Trial Two
Trial Three
0.200 grams
0.200 grams
0.200 grams
Part B
(This is for our trial one, two, and three. We kept them the same to play it safe.)
0.200 grams
1 mol NaHCO3 2 mol CO2
44.01 grams
0.105 grams
NaHCO3
CO2
CO2
(Theoretical
yield)
84.01 grams
2 mol NaHCO3 1 mol CO2
NaHCO3
Table 2: Mass of Reactants and Mass of Products
Part C
Mass of Reactants
Mass of Product
Difference in Mass
Materials
Materials
Due to Loss of CO2
Gas Produced
8.532 + 0.200 =
22.745 – 13.79 =
0.072
Trial One
8.732
8.65
2.052 + 0.200 =
15.82 – 13.79 =
0.222
Trial Two
2.252
2.03
3.024 + 0.200 =
16.96 – 13.79 =
0.054
Trial Three
3.224
3.17
This column will be
the actual yield
Part D
Trial One
(0.072 / 0.105) x 100 = 68.57 %
Trial Two
(0.222 / 0.105) x 100 = 211.43 %
Trial Three
(0.054 / 0.105) x 100 = 51.43 %
Mean = 110.48 %
Standard Deviation = 87.85
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CHE1020
Spring 2014
Commentary: Overall, I had a hard time understanding the concept of this
lab, but now after thinking about it and talking amongst classmates I have a better
understanding. I believe my group could have done a better job altogether. I believe this
because if you look at Part D, our percentages are not close, especially Trial Two. Our
Trial Two was so far off because my group didn’t take the time to actually take our time.
I also feel as if though we rushed through this lab because we messed up twice in the very
beginning of lab time.
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