Chemical Equilibrium

07.04 Equilibrium: Lab Report
Equilibrium Lab Report
Data and Observations:
Part I
ROUND
CANDIES ON R SIDE
CANDIES ON P SIDE 0
40
0
1
20
20
2
15
25
3
14
26
4
14
26
5
14
26
6
14
26
7
14
26
8
14
26
9
14
26
10
14
26
Ratio = 0.7 Part II
ROUND
CANDIES ON R SIDE
CANDIES ON P SIDE
0
20
20
1
5
10
2
2.5
2.5
3
0.6
1.5
4
0.3
0.3
5
0.8
0.15
6
0.04
0.4
7
0.1
0.02
8
0.005
0.05
9
0.03
0.003
10
0.0008
0.01
Ratio = 1.2

Calculations:

Conclusion:
Answer the following questions in complete sentences, giving detailed explanations and support for each of your answers.
1. Explain in your own words what it means for a chemical system to be in the state of dynamic equilibrium.
All reactions are able to reach equilibrium but only if they it happens in closed systems. Dynamic equilibrium is a state of balance where forward and reversed reactions happen at the same time.
2. Describe what you observed in each part of this lab. Do you think that each part of this activity helped illustrate the concepts of equilibrium? Explain your answer completely in paragraph form.
There was a pattern on while the reactants were decreasing the products were increasing, showing that the reaction is two-way. This showed that two occurrences were going on and illustrated that two reactions can happen at the same time. This was a real hands on lab for me allowing me to see and experience the meaning of equilibrium.
3. How did the calculated ratios of product to reactant compare in the three parts of this activity. Explain, in paragraph form, if these ratios illustrate the concept of the law of mass action and the equilibrium constant of a system.
4. What determines when a system reaches equilibrium? What observations can be made about a system once equilibrium has been established?
The rate of the forward reaction must equal to the backward reaction. Also, the concentration of the reactant must equal to its product.
5. What does the value, or magnitude, of the equilibrium constant (K) tell you about an equilibrium system? Be specific with your answer.
If K > 1, there will be more products and not as many reactants
It tells you that the products or reactants are favored in the equilibrium.
6. In real life, a given system can approach equilibrium from different starting points but will still have the same equilibrium constant. How is this possible? Explain your answer in complete sentences. At any temperature a reaction will have a k value (equilibrium constant), and this will stay constant. This means is that the amount of product you make will change because the k value cant.