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Part II: Answer the following stoichiometry problems showing all appropriate work.
1) How many grams of Aluminum oxide do I need to make 55.5 grams of Iron (III) oxide?
1 Fe2O3(s) + 2 Al(s) --> 2 Fe(s) + 1 Al2O3(s)
2) How many grams of glucose (C6H12O6)? do you need to "burn" biologically (see reaction below) to get 32.5L of oxygen gas @STP ?
1 C6H12O6 + 6 O2 (g) --> 6 CO2 (g) + 6 H2O1 (l)
Part III Kinetics Questions
1. What two questions about a chemical reaction does Kinetics answer?
a)
b)
2. What one question about chemical reactions does kinetics NOT answer and what chemical concept does answer this question?
3. What is the name of the theory (and give a one sentence explanation) that all of kinetics are based on? _______________________
4a. For Mr. Mr. McLeod's class, what two words must be in all answers (except reaction mechanism problems) of kinetics?__________________
4b. What are the two factors that determine the answer from Question #4a above?
a)
b)
5. On the back of this page, explain how increasing temperature increases the rate of reaction. In your explanation, use (including explaining graph) the Kinetic energy diagram as part of your explanation.
6a. On the back of this page, answer the same questions as in Q5. above except for having more reactant particles near each other per volume.
6b. Give at least two ways that you can get more reactant particles near each other per volume.
i)
ii)
7. On the back of this page, 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. What is the "sign" of deltaHrxn for an exothermic reaction. Then show on the graph and through effective collisions how adding a catalyst increases rate of the reaction.
8.Most overall chemical reactions are multi-step (ie all the reactants do not react all at once). What is the reason why this is so?
8. State the two requirement for a substance to be a catalysis.
a)
b)
9. Define what an intermediate is.
10. One mechanism for the destruction of ozone (O3) in the upper atmosphere is
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.