Analysis2291 bloy1. Write a balanced chemical equation for the reaction between acetic acid andthe sodium bicarbonate. The products are aqueous sodium acetate, liquidwater, and carbon dioxide gas.сог→ CH3COONa + H₂O +CH3COOH + NaHCO3 -2. What evidence from the lab shows that a chemical reaction took place?Explain.3. Which product was collected in your balloon? Explain.4. According to the quantities you used of the two reactants and the amount ofcarbon dioxide you produced, which is the limiting reactant?5. Look at your observations. Was there any indication that this would be yourlimiting reactant based on your observations? Explain.6. What mass of the excess reactant was left unreacted?7. What is the theoretical yield of carbon dioxide?8. What is the actual yield of carbon dioxide?9. What is the % yield of product produced in this lab?After the 10. Why was your % yield less than 100%? State one experimental error thatcould have occurred in the lab and how this contributed to your % yield.11. What was the point of taking the pH before and after the reaction? What didit tell you?Snow12. What would you have to do in this lab for the balloon to get bigger? Explainwhy this would work.91 diesWWeve do wy(baubes nu fiel asw.dns691 2290X905 g/ml,our work. Becafobixolb nedratHWiv 150106 901 eldenW 8

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Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Analysis
2291 bloy
1. Write a balanced chemical equation for the reaction between acetic acid and
the sodium bicarbonate. The products are aqueous sodium acetate, liquid
water, and carbon dioxide gas.
сог
→ CH3COONa + H₂O +
CH3COOH + NaHCO3 -
2. What evidence from the lab shows that a chemical reaction took place?
Explain.
3. Which product was collected in your balloon? Explain.
4. According to the quantities you used of the two reactants and the amount of
carbon dioxide you produced, which is the limiting reactant?
5. Look at your observations. Was there any indication that this would be your
limiting reactant based on your observations? Explain.
6. What mass of the excess reactant was left unreacted?
7. What is the theoretical yield of carbon dioxide?
8. What is the actual yield of carbon dioxide?
9. What is the % yield of product produced in this lab?
After the

10. Why was your % yield less than 100%? State one experimental error that
could have occurred in the lab and how this contributed to your % yield.
11. What was the point of taking the pH before and after the reaction? What did
it tell you?
Snow
12. What would you have to do in this lab for the balloon to get bigger? Explain
why this would work.
91 diesW
Weve do wy
(baubes nu fiel asw.dns691 2290X9
05 g/ml,
our work. Beca
fobixolb ned
rat
HW
iv 150106 901 eldenW 8

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The addition of stoichiometric coefficients to the reactants and products is necessary to balance chemical equations. This is significant because a chemical equation must adhere to the laws of conservation of mass and constant proportions, meaning that both the reactant and product sides of the equation must contain the same number of atoms of each element.

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