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24 Cards in this Set
- Front
- Back
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Calorimetry
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the measure of heat exchange
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Energy is either...
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a reactant
a product |
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If a rxn requires energy from the surroundings it...
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Gets cold
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If a rxn gives off energy to the surroundings it...
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Gets hot
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1st Law of Thermodynamics
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Energy cannot be created nor destroyed
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Exothermic
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Products have less chemical energy than reactants
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Endothermic
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Products have more chemical energy than reactants
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System
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Reaction area
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Surroundings
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Everything except the reaction area
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Heat capacity
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the amount of heat energy needed to raise a system by 1°C
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Heat Capacity (units)
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Heat absorbed/
∆T J/°C |
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Heat Energy
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Heat capacity*∆T
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Specific Heat
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the amount of energy required to raise 1g of material by 1°C
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Specific Heat (units)
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J/
g°C |
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Amount of heat in a system
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specific heat*mass*∆T
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Calorimetry
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Take known system (mass and specific heat) and measure the temperature change as a result of a reaction
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Qr=
Qs= |
Qr= heat of rxn
Qs= heat of surroundings Qr=-Qs Qr= Csp*mass*∆T |
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Specific heat of water
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4.184 J/g°C
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Change in Energy
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E final-E initial
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Enthalpy
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Chemical energy
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Change in enthalpy
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∆H=H final- H initial
∆H=H products- H reactants |
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∆H > 0
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-products have more energy than reactants
-energy entered the system -endothermic |
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∆H < 0
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--products have less energy than reactants
-energy left system -exothermic |
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State Function
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independent of pathway
*mountain analogy* |
