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Definition
| The study if relationships between chemistry and energy. |
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Term
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Definition
| The flow of energy due to temperature difference. |
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| What is the difference between energy and heat? |
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Definition
| Heat is the flow of thermal energy, whereas energy is something that can be possessed. |
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Term
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Definition
| Energy associated with motion. |
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Definition
| Kinetic energy associated with the motion of atoms or molecules within a substance. |
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Definition
| The energy associated with the position of composition of an object. |
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| Law of the conservation of energy |
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Definition
| Energy can neither be created nor destroyed, but it can be transferred or transformed. |
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Term
| Raising a ball of a table makes _________ energy, whereas dropping it changes it to ____________ energy. |
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Definition
| Raising a ball off a table makes potential energy, whereas dropping it changes it to kinetic energy. |
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Term
| The first law of thermodynamics |
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Definition
| the total energy in the universe is constant. |
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| True or false: at least as much energy must go into something as comes out of it. |
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Definition
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Term
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Definition
| The sum of the kinetic and potential energy of a system. |
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Term
| Two kinds of state functions |
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Definition
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Term
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Definition
| The value of energy depends only on its state and not on how it arrived at that state. |
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Term
State the relation between:
Delta-E-system
Delta-E-surroundings |
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Definition
| Delta-E-system = -(Delta-E-surroundings) |
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Term
| How may a system exchange energy with its surroundings? |
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Definition
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Term
| Energy leaving the system is ___________ |
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Definition
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Term
| Energy entering the system is ___________ |
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Definition
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Term
| While the internal energy is a _________ __________, heat and work are ________ ___________ |
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Definition
| While the internal energy is a state function, heat and work are path functions. |
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Term
Define the relation between:
Delta-E-system
Delta-E-surroundings
O |
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Definition
| Delta-E-system - Delta-E-surroundings = 0 |
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Term
| Quick way to see state and path |
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Definition
| State is uppercase, path is lowercase. |
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Term
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Definition
| The measure of thermal energy |
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Term
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Definition
| Done without heat (So not change in temperature). |
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Term
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Definition
| Amount of heat required to raise 1 gram of water by 1*C |
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Term
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Definition
| The amount of heat required to raise the temperature of 1 gram of a substance by 1*C. |
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Term
| Specific heat is an _____________ measure. |
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Definition
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Term
| Specific heat can be applied to any substance as long as you know __________________ |
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Definition
| the mass of the substance. |
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Term
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Definition
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Term
| How is specific heat represented? |
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Definition
| Cs, c, s (Most commonly c for Porter) |
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Term
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Definition
| The heat required to raise the temperature of a substance by 1*C |
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Term
| Heat capacity is an ____________ measure. |
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Definition
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Term
| Heat capacity can be applied to ____________________________. |
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Definition
| Only a particular sample. |
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Term
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Definition
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Term
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Definition
| The amount of heat required to raise the temperature of 1 mole of a substance by 1*C |
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Term
| Units of molar heat capacity |
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Definition
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Term
| Symbol for molar heat capacity |
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Definition
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Term
| A substance with the smallest specific heat in a group given the same amount of thermal energy will end up with _______________ |
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Definition
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Term
| In regards to deltas, one should not |
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Definition
| Convert them to different units after you find you've worked them out. |
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Term
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Definition
| Compression of expansion of gases. |
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Term
| If a gas expands, work is ____________. |
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Definition
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Term
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Definition
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Term
| What units does the work formula produce? |
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Definition
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Term
| Heat is equal to internal energy when... |
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Definition
| There is no change in volume, and therefore no work done. |
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Term
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Definition
| The measurement of heat involved in a chemical reaction by observing the temperature changes in the surroundings |
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Term
| Symbol for heat absorbed by calorimeter |
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Definition
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Term
How do these stand in relation to one another:
qcal
qrxn |
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Definition
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Term
| The amount absorbed by a calorimeter is ___________ to the amount released in the reaction. |
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Definition
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Term
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Definition
| The amount of heat released at constant pressure (AKA: Open to the atmosphere). |
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Term
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Definition
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Term
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Definition
| A balanced Chemical equation. |
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Term
| Bomb calorimetry occurs at ______________________ and measures __________________ for a reaction |
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Definition
| Bomb calorimetry occurs at constant volume and measures change-in-internal energy for a reaction. |
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Term
| Coffee cup calorimetry occurs at _________________________ and measures ______________ of a reaction |
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Definition
| Coffee cup calorimetry occurs at constant pressure and measures change-in-ethalpy |
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Term
| Change in H is a measure of... |
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Definition
| The heat exchanged under constant pressure. |
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Term
| When are change in internal energy and change in enthalpy nearly identical? |
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Definition
| When a reaction does not cause a large change in volume, so that the change in internal energy is in the form of q and not w. |
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Term
| Postive H is an __________________ reaction |
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Definition
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Term
| Example of an endothermic reaction |
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Definition
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| Negative H is an _________________ reaction |
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Definition
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Term
| Example of an exothermic reaction |
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Definition
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Term
| What is the source of thermal energy in an exothermic reaction? |
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Definition
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Term
| What happpens to absorbed thermal energy in an endothermic reaction? |
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Definition
| It becomes potential energy. |
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Term
| Ethalpy is a ______________ measure |
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Definition
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Term
| Ethalpy is defined in a _________________________ |
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Definition
| ratio with moles from a balanced chemical equation. |
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