Kinetics and Rates
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| Define the collision theory | When two chemicals react, their molecules have to collide with each other with proper energy and orientation
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| What is the probability that two molecules will react? | The chance of the collision in the proper orientation with the proper energy is about 1/2.
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| Will five molecules in the same equation ever react in one step? | No, the probability is almost impossible!
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| What are elementary steps? | Series of smaller steps that eventually lead to the overall reaction.
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| Define intermediates | Species that are created during the elementary steps of the reaction, but are not a part of the overall reaction. They are products, and they are consumed as reactants immediately.
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| What are catalysts? | Catalysts speed up chemical reactions by decreasing the activation energy required. They are reactants, and they come out as products in the overall reaction.
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| Reaction mechanisms are the ones that determine the rate law because they are | slow
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| What is activation energy? | The amount of energy required to initiate a chemical reaction. In exothermic reactions, the overall will be greater than the initial, and in endothermic, it will be less than the activation energy.
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| Zero order reactions are not dependent on | concentration
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| The graph for zero order reactions are: | rate=k
(-k)
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| In second order reactions if the concentration doubles the rate will | quadruple
or do the square of what the concentration did
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| The graph for second order reactions are: | t vs. 1/(A) and the slope= k
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| In first order reactions if the concentration doubles the rate will | double
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| The graph for first order reactions are: | t vs. ln(A) and the slope is -k
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| What equation will be used to find the activation energy? | Arrhenius' Equation
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| Which factors affect the rate? | Temperature, surface area, concentration, the use of catalysts, if the compound is ionic, or if it is in aqueous form
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| How are rate laws determined (experimentally or theoretically)? | Using experimental data, so experimentally
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| Why do ionic substances react faster? | They break into ions, unlike covalent substances
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| How do you determine the overall reaction order? | Add all the exponents of the orders together for the overall
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| Write the rate law for a first order reaction using A and B, if the rate doubles when A is doubled, and the rate stays the same when B doubles | rate= k(A)^1(B)^0
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| Write the basic steps used to find slopes in a calculator | 1. Stat, Edit
2. Enter Data
3. Stat, Calc
4. LinearRegression
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| The rate law graphs correspond to which easy, and famous graph? | Linear graphs
y= mx +b
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| What are unimolecular reactions? | When only one molecule is reacting.
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| What are bimolecular reactions? | When two molecules are reacting.
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| What are termolecular reactions? | When three molecules are reacting.
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| Why are termolecular reactions uncommon? | The chances of two molecules reacting are only 1/2, three are even less than that.
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| Is 2NO + O a bimolecular or termolecular reaction? | Termolecular because there are three molecules in total. The coefficient must be accounted for.
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