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28 Cards in this Set
- Front
- Back
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Calorie |
this is the quantity of the heat needed to raise the temperature of 1 gram of pure water 1 degree Celsius. |
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Calorimeter |
insulated device used to measure the absorption or release of the heat in chemical and physical processes. |
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Calorimetry |
accurate and precise measurement of heat changes for chemical and physical changes. |
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Chemical Potential Energy |
energy stored within the structural units of chemical substance. |
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Endothermic Process |
absorbs heat from the surroundings; system gains heat as the surrounding cool down; q is positive. |
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Energy |
capacity to do work. |
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Enthalpy |
heat of the system; H; the heat content of a system at constant pressure; q= delta H; Delta H = m*C*delta T; C= delta T; C= q/m*delta T C=delta H/m*delta T; Delta H= the heat change m= mass C= specific heat delta T= temp final-temp initial if delta H is negative then it is an exothermic reaction; if delta H is positive it is an endothermic reaction. |
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Exothermic Process |
releases heat to its surroundings, system loses heat as the surrounding heat up. q is negative (-) |
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Heat |
energy that transfers from one object to another because of the temperature difference. (q) |
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Heat Capacity |
amount of heat needed to increase the temperature of an object at exactly 1 degree Celsius. |
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Heat of Combustion |
the heat of reaction for the complete burning of 1 mole of substances; (delta H combination) |
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Heat of Reaction |
the heat change for the equation exactly as it is written |
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Hess's Law of Heat Summation |
if you add 2 or more thermochemical equations to give a final equation then you can add the heats of the reaction to give the final heat of reaction |
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Joule |
SI unit of heat needed to increase the temperature of an object at exactly 1 degree Celsius. 1 Joule= .2390 calories; 1 calorie= 4.184 Joules |
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Law of Conservation of Energy |
energy is neither created nor destroyed but accounted for as work, stored, energy, or heat. |
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Molar Heat of Condensation |
the amount of heat released when 1 mole of vapor condenses; delta H vap delta H vap= - delta H cond ALWAYS NEGATIVE g -> l |
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Molar Heat of Fusion |
the heat absorbed by 1 mole of a substance in melting from a solid to a liquid at a constant temp; delta H fus ALWAYS POSITIVE s -> l |
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Molar Heat of Solidification |
the heat lost when 1 mole of a liquid solidifies at a constant temp; delta h solid ALWAYS NEGATIVE l -> s |
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Molar Heat of Solution |
the heat change caused by the dissolving of 1 mole of a substance; delta H soln If delta H soln is a reactant = endothermic If delta H soln is a product = exothermic |
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Molar Heat of Vaporization |
the amount of heat necessary (absorbed) to vaporize 1 mole of a given liquid; delta H vap ALWAYS POSITIVE l -> g |
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Specific Heat |
the amount of heat it takes to raise the temperature of 1 gram of the substance at 1 degree Celsius. Independent of the masses; "C" |
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Specific Heat Capacity |
the amount of heat it takes to raise the temperature of 1 gram of the substance at 1 degree Celsius. Independent of the masses. "C" |
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Standard heat of Formation |
the change in enthalpy (heat) that goes with the formation of 1 mole of a compound from its elements with all substances in their standard states (solid, liquid, gas) at 25 degrees Celsius; (delta H degree f) of a free element (off the chart) is set to zero kj/mol. |
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Surroundings |
everything else not in the system. |
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System |
part of the universe on which attention is focused. |
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Thermochemical Equation |
an equation that includes the heat change; if the heat is a reactant the reaction is endothermic and positive when using the number in the equation; if the heat is a product the reaction is exothermic and negative when used in the equation. |
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Thermochemistry |
concerned with the heat changes that occur during a chemical reaction |
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Universe |
system and the surroundings. |
