Term
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Definition
| The rate of change if a product in a chemical reaction |
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Term
Closed book part of test
Define heterogenous catalyst |
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Definition
| Catalysts that are in a different phase than the reactants |
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Term
Closed book part of test
Define homogenous catalyst |
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Definition
| A catalyst that has the same phase as at least one of the reactants |
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Term
Closed book part of test
How can you speed up a reaction rate? |
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Definition
| You can speed it up with heat, increased surface area, or increased concentration of reactants |
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Term
Closed book part of test
Explain how heat can speed up a reaction |
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Definition
| Reactant molecules move faster as the heat increases which increases the chances of atoms colliding into each other and electrons can be rearranged or transferred |
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Term
Closed book part of test
Explain how increasing concentration of chemical reactants |
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Definition
| There will be more molecules to collide into with and therefore electrons can be rearranged or transferred |
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Term
Closed book part of test
Explain how increasing surface area increases rate reaction |
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Definition
| Molecules or atoms can more easily mingle with the other moecules or atoms. |
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Term
Closed book part of the test
Understand rate orders
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Definition
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Term
Closed book part of the test
example of rate orders:
2ICl +H2 --> I2 + 2HCl
The following reaction is determined to be first order with respect to 2HCl and H2 is determined to be zero order. What does that mean |
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Definition
H2 has no effect on the reaction and it would be written as:
R= k(2HCl)
I2 would be dropped since it has no effect on the equation |
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Term
Closed book part of the test
example of rate orders:
2N2 + 3H2 --> 2NH3
The following reaction is determined to be second order with respect to 2N2 and first oder with respect to 3NH3 What is the overall equation |
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Definition
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Term
| How is the temperature of a chemical reaction shown in a rate equation? |
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Definition
| The rate constant (k) is dependent on the temperature of chemical reaction |
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Term
Closed book part of the test
Understand activation energy and how it effects a reaction rate.
Example;
If you have 2 different reactions but they both have the same the activation energy, what does that say about each of the reaction rates
B. If there are 2 different reactions but only the first one has a catalyst to speed up the reaction. Which reaction has a lower activation energy?
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Definition
A. The reaction times would be the same
B. The first one has a lower activation energy because the catalyst lowers the activation energy. |
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Term
Closed book part of the test
Understand catalysts
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Definition
| Catalysts speed up the reaction rate without actually getting used up in the chemical reaction. |
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Term
Open book part of the test
Study the examples in the book
14.1 page 465
14.2 pages 466-468
14.3 pages 469-471 |
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Definition
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Term
Open book part of the test
Study how chemical reactions double for every 10°C increase in temperature.
study example 14.4 page 478 |
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Definition
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