Editing revision 6 of Review Homework For Equilibrium Test

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1. 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 <nowiki>([ ])</nowiki> vs. time, show where equilibrium occurs and explain it in macroscopic term (looking at the overall bucket) and microscopic term (following one particle). c. What is the phrase Mr. <nowiki>McLeod</nowiki> uses so you know what is in your bucket at equilibrium? 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
2. 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. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
3. 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. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
4. 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). 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
5. 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, 75% of <nowiki>NO</nowiki> has reacted. Calculate the equilibrium concentrations of all the species (called equilibrium position) and K (include units of K) for this reaction. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
10. At a given temperature, the reaction below has a K = 2.50 
1 SO2(g) + 1 NO2(g) <==> 1 SO3(g) + <nowiki>NO</nowiki>(g)

If all four gases had an initial concentration of 1.00M, calculate the equilibrium concentration of all species. 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
11. The industrial production of ammonia is described by this reversible reaction 
1 N2(g) + 3 H2(g) <==> 2 <nowiki>NH</nowiki>3(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. addition of heat 
b. removal of <nowiki>NH</nowiki>3 
c. decrease of pressure 
d. addition of a catalyst 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
Problem 8 : K = 9.89E-4 M2 
Problem 9 : K = 0.11 M 
Problem 10 : <nowiki>[SO</nowiki>3<nowiki>]</nowiki>E = 1.22M, <nowiki>[NO]</nowiki>E = 1.22M, <nowiki>[SO</nowiki>2<nowiki>]</nowiki>E = 0.776M, <nowiki>[NO</nowiki>2<nowiki>]</nowiki>E = 0.776M

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