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16 Cards in this Set
- Front
- Back
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thermochemistry
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the study of the transfers of energy as heat that accompany chemical reactions and physical changes.
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calorimeter
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measures the energy absorbed or released as heat in a chemical or physical change.
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temperature
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a measure of the average kinetic energyof the particles in a sample or matter.
measurement of heat. |
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joule
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the SI unit of heat as well as all other forms of energy.
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heat
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- direction of energy
- transfer of heat - high --> low - you never get cold, you only lose heat |
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specific heat
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the amount of energy required to raise the temperature of one gram of substance by one celcius degree or by one kelvin.
- conductors and insulators - conductors = low specific heat ex. gold, lead - insulators = high specific heat (holds onto energy) ex. water, glass |
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Cp= q/(m * delta T)
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specific heat (J/g*K) = energy lost or gained (J)/ mass(g) * change in temp
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heat of reaction
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the quantity of energy released or absorbed as heat during a chemical reaction. (kJ/mol)
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thermochemical reaction
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an equation the includes the quantity of energy released or absorbed as heat during the reaction as written.
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enthalpy change
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the amount of energy absorbed or lost by a system as heat during the process at constant pressure
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exothermic reaction
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- energy is released
- the q is negative |
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endothermic reaction
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- energy is absorbed
- the q is positive - tend to be more unstable |
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molar heat of formation
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the energy released or absorbed as heat when one mole of a compound is formed by combination of its element.
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enthalpy change/ delta H of elements in their standerd state
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0
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heat of combustion
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the energy released as heat by the complete combustion of one mole of a substance.
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hess's law
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the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process.
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