Editing Review Homework For Kinetics And Equilibium Test

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Please answer the following questions in an appropriate manner including showing all mathematical work, using clear concise and complete sentences and use graphs/figures as needed. 
 
1. Using the Kinetic Energy diagram, explain one of the ways that you can increase the rate of a chemical reaction.

2. Draw the potential energy diagram for an exothermic reaction and define each section of the diagram. Show where the heat of reaction deltaHrxn is located on the graph and explain how you calculate it. Then show on the graph and through effective collisions how adding a catalyst increases rate of the reaction.

3. A one liter (1L) container holds 1.45moles of nitrogen gas and 0.650mole of oxygen gas. What is the equilibrium concentration of all the species if the equilibrium constant is equal to 1.25 (K=1.25) for the following balanced chemical reaction, 
<center>1 N2 (g) + 1 O2 (g) <==> 2 NO(g)</center>

4. Carbon disulfide can be made by the reaction of carbon dioxide and sulfur trioxide by the following reaction, 2 <nowiki>SO</nowiki>3(g) + 1 <nowiki>CO</nowiki>2(g) + heat <==> 1 <nowiki>CS</nowiki>2(g) + 4 <nowiki>O</nowiki>2(g)

a. Initially I have 2.0 moles of <nowiki>CO</nowiki>2 and 8 moles of <nowiki>SO</nowiki>3 in a 1-L container. At equilibrium, 45% of the <nowiki>CO</nowiki>2 is left, what are the equilibrium concentrations for all the species (if taken as a group, you call it the equilibrium position) and Keq?

b.If you increase the temperature of this equilibrium, how will the equilibrium shift? (Hint: What would <nowiki>LeChatlier say</nowiki>) 
 
 
Answers: 
1. Will discuss in class 
2. Will discuss in class 
3. <nowiki>[NO</nowiki>] = 0.665M, <nowiki>[N</nowiki>2] = 1.11M , <nowiki>[O</nowiki>2] = 0.317M 
4. a. <nowiki>[CO</nowiki>2] = 0.90M, <nowiki>[SO</nowiki>3] = 5.8M , <nowiki>[CS</nowiki>2] = 1.1M , <nowiki>[O</nowiki>2] = 4.4M , and Keq = 13.6, units = M2 
b. Will discuss in class.

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