O3(g) + NO(g) --> NO2(g) + O2(g) Slow
NO2(g) + O(g) --> NO(g) + O2(g) Fast
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O3(g) + O(g) ---> 2 O2(g) Overall Reaction
(It may be easier to answer a & b if you first thing about the definitions)
a. Which species are catalysts.
b. Which species are intermediate.
c. I did some experiments and found that if I increased the concentration of O3, the rate of reaction increased and if I increased the concentration of O(g), the rate of reaction also would increase. Does the above reaction mechansim support this data or not? Explain.
4. a) What is the main difference between an irreversible and reversible reaction? (Hint: at infinite time, what is in your bucket?)
b) On a graph of concentration ([ ]) vs. time, show where equilibrium occurs and explain it in macroscopic term (looking at the overall bucket) and microscopic term (following one particle).
5. What are the two ways that you can write the equilibrium constant expression (hint, qualititively & quantatively). The equilibrium constant is important because it is considered a predictive quantity (i.e. it helps to explain what is going to happen). Please explain what this means including what the three difference ranges of the K value mean.
6. Using the theory of all systems want to go to the lowest energy state, explain your answer to question 4 of this homework (a diagram will help). Is it possible to initially put only product in your bucket, and why can you or can't you?(2013-2014 Do not Do this Question
7. In your own words, please provide an outline on how to calculate equilibrium problems. Do not use complete sentences, just phrase and make sure to separate the procedures for doing the math for the three major types of equilibrium problems.
8. The reaction below reaches equilibrium in a 0.25L container.
2 SO3(g) + 1 CO2(g) <==> 1 CS2(g) + 4 O2(g)
An analysis of the equilibrium mixture gives the following results:
SO3(g) 0.053mol, CO2(g) 0.106mol, CS2(g) 0.047mol, O2(g) 0.025mol.
Calculate K for this reaction (also give units of K).
9. At a particular temperature, 8.0mol NO2 is placed in a 1.0L container and the NO2 dissociates by the reaction:
2 NO2(g) <==> 2 NO(g) + 1 O2(g)
At equilibrium, the concentration of NO is 2.0M. Calculate K for this reaction.
If all four gases had an initial concentration of 1.00M, calculate the equilibrium concentration of all species.
(For 2011-2012 Can Not Do This Problem)
11. The industrial production of ammonia is described by this reversible reaction
1 N2(g) + 3 H2(g) <==> 2 NH3(g) + Energy
Using the 4 part explanation for how Le Chatlier's Principle would explain how the system would be affected by the following stresses:
a.Stress: Addition of heat (increase temp)
How rxn tries to remove stress: _________________________________________________
Circle: Make more product or more reactant
Circle: Favoring: Forward rxn or Backward rxn
Circle: Shift Equilibrium to: Left(more reactant) or Right (more product)