In a model experiment baking soda (sodium bicarbonate) is combined with white vinegar (5% acetic acid) under the following circumstances:
Sodium bicarbonate + acetic acid → carbon dioxide + water + sodium acetate
NaHCO3 (s) + CH3COOH (l) → CO2 (g) + H2O (l) + NaCH3COO (aq)
1. What are the “reactants” in this reaction?
2. What “forms” are the reactants each in?
3. What are the “products” in this reaction?
4. What “forms” are each product in this reaction found in?
5. Is this equation balanced? Why or why not?
6. If I told you this reaction is “endothermic” and you touched the bottom of the catch tray after the reaction runs would it feel hot or cold? Why?
7. If I increase the amounts of both reactants would you expect the reaction to speed up or slow down? Why?
8. If I increase the amount of one reactant only, what would you expect to happen? Why?
9. How do I know that carbon dioxide is being produced? What is my “direct observation”?
10. If I went to the store and purchased apple cider vinegar which has a known concentration of 10% acetic acid and used it in place of white vinegar, what variable am I altering and what result would you expect?
11. If I tried this experiment with baking soda that had been open and in my refrigerator for two months and was still “cold” when I started the experiment, what results might we expect? Why?
12. If I was setting up my experiment and I carefully allow both the baking soda and vinegar to reach room temperature before I started my experiment - what part of an experimental design would I be affecting? Select one.
a. Independent variable
b. Dependent variable
c. Constant
d. Control
13. If I warmed my vinegar to a temperature of 85℉ from room temperature of 72℉, what result would you expect and why? Select one.
a. The reaction would proceed faster as you could see from more rapid foaming because there are more particle collisions between warmer reactants.
b. The reaction would proceed faster as you could see from more rapid foaming because there are fewer particle collisions between warmer reactants.
c. The reaction would proceed more slowly because there are more particle collisions between warmer reactants.
d. The reaction would not proceed because the activation energy wouldn’t be reached.
14. If I used laboratory grade acetic acid (100% concentration) describe how the following variables would change:
a. Concentration of reactants (independent variable) -
b. Formation of products (dependent variable) -
c. Rate of reaction (slope of the line) -
15. If this sample “unlabelled graph” were used from this experiment - how could we label each portion of the graph? What type of relationship do we see?
if you wanna see the graph then go to this brainly link: h t t p s : / / b r a I n l y . c o m / q u e s t i o n / 3 1 0 4 9 5 7 7
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oh btw it got answered on brainly
1. The reactants in this reaction are sodium bicarbonate (NaHCO3) and acetic acid (CH3COOH).
2. Sodium bicarbonate is in solid form (s), and acetic acid is in liquid form (l).
3. The products in this reaction are carbon dioxide (CO2), water (H2O), and sodium acetate (NaCH3COO).
4. Carbon dioxide is in gaseous form (g), water is in liquid form (l), and sodium acetate is in aqueous form (aq).
5. No, this equation is not balanced. There are 2 hydrogen atoms on the reactant side but only 1 hydrogen atom on the product side, so it needs to be balanced by doubling the water molecule:
NaHCO3 (s) + 2 CH3COOH (l) → CO2 (g) + 2 H2O (l) + NaCH3COO (aq)
6. If the reaction is endothermic and you touch the bottom of the catch tray after the reaction runs, it would feel cold. This is because endothermic reactions absorb heat from the surroundings, so the temperature of the surroundings decreases.
7. Increasing the amounts of both reactants would likely speed up the reaction. This is because an increase in reactant concentration leads to more frequent collisions between reactant particles, increasing the chances of successful collisions and speeding up the reaction.
8. If you increase the amount of one reactant only, the reaction may still proceed, but at a slower rate. This is because the reaction rate is determined by the concentration of the reactants, and increasing the concentration of only one reactant would limit the number of available reactant particles, leading to a slower reaction rate.
9. To know that carbon dioxide is being produced, the direct observation would be the formation of bubbles or foaming. Carbon dioxide gas is released during the reaction, and the formation of bubbles indicates its production.
10. If you use apple cider vinegar instead of white vinegar, you would be altering the concentration of acetic acid in the reaction. Since apple cider vinegar has a higher concentration of acetic acid (10% compared to 5% in white vinegar), you would expect a more vigorous reaction with increased foaming and faster production of the products.
11. If you used baking soda that had been open and in the refrigerator for two months and was still "cold" when you started the experiment, you might expect a slower or weaker reaction. Baking soda can absorb moisture from the air over time, which may lead to a decrease in its reactivity. Additionally, exposure to the cold temperature of the refrigerator could further slow down the reaction.
12. If you allow both the baking soda and vinegar to reach room temperature before starting the experiment, you would be affecting the Constant in the experimental design. Keeping the temperature of the reactants constant is a way to control and stabilize the conditions during the experiment.
13. The correct answer is a. The reaction would proceed faster as you could see from more rapid foaming because there are more particle collisions between warmer reactants. Increasing the temperature of the vinegar to 85℉ would result in faster reaction kinetics. Higher temperature means higher average kinetic energy of the reactant particles, leading to more frequent and energetic collisions, which speeds up the reaction.
14. a. By using laboratory grade acetic acid with 100% concentration, the concentration of reactants would increase significantly. This may result in a more vigorous reaction.
b. The formation of products would not be affected by using laboratory grade acetic acid. The same products (CO2, H2O, NaCH3COO) would still be formed.
c. The rate of reaction (slope of the line) would increase. The higher concentration of reactants would lead to more collisions and a higher reaction rate.
15. Without the ability to view the graph, I am unable to provide specific labels for each portion. However, typically, you can label the x-axis as "Time" and the y-axis as "Amount of Product" or "Reaction Rate." The graph may show an increase in the amount of product formed over time, indicating a positive relationship between the reaction progress and the measured variable.