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07.04 Equilibrium

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fa lee

on 9 March 2015

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Transcript of 07.04 Equilibrium

07.04 Equilibrium
Round Candies on R side Candies on P side
Part 2
Round Candies on R side Candies on P side
Part 3


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.
An equilibrium in a particular state exists in a physical or a chemical reaction when there is no change seen as the forward rate reaction and reverse reaction are the same. Dynamic equilibrium is really a balance state where the reverse and the forward reactions take place at the same time, and their rates are the same as well. Both the forward and the reverse reaction are kept the same with time, and there is no change because of this. Every reaction can reach equilibrium, but only if they take place in closed systems.

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.
In this specific lab, I recognized that there will be a pattern that while the reactants were minimizing, the products began increasing. This particular situation displays that this reaction is two-way. It also helped represent a certain state of being where the rate of the formation of products becomes equal to that of the reactants. I believe that this activity did aid in representing the concept of equilibrium. As it was mentioned before, the reactants began to minimize while the products began to get larger. This showed that two things were happening, thus it expressed where the reverse and forward reactions can take place at the same time, with equal rates. It would reach the equilibrium state when the numbers started to repeat. It gave me a real-hands on activity where I was able to see, physically participate, and experience the concept 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.
All reactions show that 2 moles of product are yielded from 1 mole of reactant or 1mole of 2 products come from 1 mole of reactant. for example: N2O4 = 2 NO2. You have 3 reactions with the assumption that the rxn occurs at a constant temp, all ratios of products:reactants = 2


Conclusion:
Part 1
Round Candies on R side Candies on P side
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The sum of the product is 348 , divided by 331, the sum of the reactant is 1.05
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The sum of the product is 227 , divided by 213, the sum of the reactant is 1.07
The sum of the product is 227, divided by 213, the sum of the reactant is 1.07
4.What determines when a system reaches equilibrium? What observations can be made about a system once equilibrium has been established?
The rate of reaction in the forwad reaction must be the same to the backward reaction and also the concentration of the reactant must equal to its product. Once equilibrium has reached no new product is formed in the forwad reaction and the mass doesn't change in the individual products

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, reactants will be in higher concentrations.
If K << 1, mostly reactants and not many products.
If K > 1, products will be in higher concentrations.
If K >> 1, mostly products and not many reactants.

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.
No matter where the system starts, it will reach an equilibrium state when the equilibrium ratio is reached.
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