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| Why do we study energy in chemistry? |
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Definition
| Everything involved in chemistry also involves energy, such as phase or chemical changes. |
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| capacity or ability to do work |
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| moving an object using a force |
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| energy of position or condition |
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| chemical potential energy |
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Definition
| energy stored within chemicals because of their composition (the energy is stored within bonds and attractions) |
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Definition
| form of energy that flows from areas of high temperature to areas of low temperature; real; dependent on amount |
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| relative heat content; average kinetic energy; not real |
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| Law of Conservation of Energy |
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Definition
| In an ordinary chemical or physical change, energy cannot be created or destroyed; it changes form. |
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| amount of heat needed to raise the temperature of one gram of water one degree Celsius |
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| Calorie (Cal) or kilocalorie (kcal) |
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| food calorie; 1000 calories |
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| any part of the universe that the attention is focused on; what you are studying |
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| the remainder of the universe that outside the system; especially the air surrounding the system, et cetera |
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| any reaction that takes in energy from its surroundings, any reaction with a positive delta H |
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| any reaction that puts off energy to the surroundings; any reaction with a negative delta H |
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| the minimum energy colliding particles must have to react |
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| a substance that speeds up a reaction without being used up; a substance that makes particles move closer together, thereby increasing the chances of the particles hitting each other and reacting and lowering activation energy |
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Definition
| products-reactants; enthalpy; heat of reaction |
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| amount of heat required to raise the temperature of one gram of a substance by one degree Celsius |
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| If you add two or more thermochemical equations to give a final equation, you can also add the heat changes to give a final heat change. |
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| What do you do to delta H when you flip the equation associated with it? |
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Definition
| multiply delta H by negative one or flip the charges |
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| When you multiply an equation, what do you do to the delta H value associated with it? |
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Definition
| multiply it by the same amount. |
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| What does q represent in the calorimetry equation? |
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Definition
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Term
| What does m represent in the calorimetry equation? |
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Definition
| mass of the object with a heat change in grams |
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Term
| What does C represent in the calorimetry equation? |
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Definition
| specific heat of the object with the heat change in Joules/(grams*degrees Celsius) |
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| What does delta T represent in the calorimetry equation? |
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Definition
| temperature change in degrees Celsius, (final temperature-initial temperature) |
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| conversion factor between Joules and calories |
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Definition
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| conversion factor between calories and Joules |
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