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Definition
| the average kinetic energy of its particles |
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| amount of KE that flows from a hot object to a cold object as a result of their difference in temperature. |
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Definition
| the sum of energy of all of the individual particles |
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Definition
| depends only on an object's current state; we only care about final - initial |
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Definition
| pressure, temperature, volume, and chemical composition |
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Term
| Equation: Heat and temperature |
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Definition
Q = (C)*∆T = (m*s)*∆T
Heat = heat capacity * temp
Heat = specific heat * mass * temp |
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Definition
J/(°C)
amount of energy needed to raise the temperature of an object by 1°C |
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Definition
J/(g°C)
the amount of heat required to raise the temperature of 1 gram of a substance by 1°C |
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Definition
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Definition
| Produces heat; products have less PE (and more KE) than reactants. Weak bonds form strong bonds, which hold less PE because they're smaller |
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Term
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Definition
| Absorbs heat; products have more PE (and less KE) than reactants |
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Definition
| The amount of heat absorbed or released in a reaction; determined by measuring ∆T |
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Definition
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Definition
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Term
| Equation: Internal energy change |
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Definition
∆E = w + Q
The change in internal energy is equal to the work and heat that goes into the system |
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Definition
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Term
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Definition
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Term
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Definition
∆H = Q when ∆P = 0
The change in enthalpy is equal to the change of KE (heat) at constant pressure |
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Term
| Difference between ∆E and ∆H |
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Definition
| large in gasses, insignificantly small in gas/ solid |
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Term
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Definition
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Term
| Standard Heat of Reaction (∆H°) |
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Definition
| the value of ∆H for a reaction in reactants and products in their standard conditions; involves the actual numbers of moles specified by the coefficients of the equation |
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Term
| Equation: Change in enthalpy at standard pressure |
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Definition
∆H = ∆E + P∆V = Qp
change in enthalpy is the change in energy minus the work done by the system.
At standard pressure, change in enthalpy is the change in heat |
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Term
| Standard Enthalpy of Formation (∆H°f) |
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Definition
| the change in enthalpy for a reaction that forms one mole of the compound from its elements, with all substances in their standard states. |
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Term
| The standard enthalpy of formation (∆H°f) of the most stable form of any element: |
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Definition
| zero; no formation reaction needed when the element is already in its standard state |
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Term
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Definition
| change in heat energy (∆H), reaction-induced change in heat energy when reactants and products in their standard conditions (∆H°), forms 1 mole of compound from its elements with everything in most stable state (∆H°f) |
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Definition
| The change in chemical potential energy in a reaction |
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Term
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Definition
w = -P∆V
Work is the pressure times the change in volume |
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