the average kinetic energy of the particles inside
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Heat capacity
the capacity or absorbing ability a system has for heat energy
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Specific heat capacity
the amount of energy that the given mass of a substance can absorb to produce 1C increase in temperature
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Enthalpy
the change from chemical energy to heat energy
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Enthalpy of fusion
The energy required to overcome the forces holding the particles together in a solid. Always endothermic.
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Enthalpy of vaporation
The energy required to separate the particles in a liquid. Always endothermic.
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Enthalpy of combustion
the energy released when 1mol of substance burns in excess oxygen
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Enthalpy of formation
the energy change when 1mol of substance is formed from its constituent elements in their standard state
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Enthalpy of neutralization
the energy released when 1mol of water is formed by the reaction between an acid and a base in an aquas solution
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Enthalpy of solution
the energy change when 1mol of substance is dissolved in a solution to infinite dilution
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Enthalpy of reaction
the energy change when a reaction proceeds to completion in the stoichiometric amounts as expressed in the equation
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Hess' Law
the enthalpy change for any chemical reaction is independent of the route, provided the starting conditions and final condition, and reactants and products, are the same
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Bond enthalpy
the energy required to break 1mol of specific bonds in a specific molecule in gaseous state under standard conditions (particular type of bond in a unique molecule)
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Lattice enthalpy
the energy required to break 1mol of ionic lattice into its individual constituent ions to infinite seperation
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Average bond enthalpy
the average amount of energy needed to break a specific type of bond measured over a wide variety of different molecules
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Standard state of a substance
the pure form of the substance under standard conditions
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First electron affinity
the enthalpy change when 1mol of gaseous atoms attract 1mol of electrons
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Entropy
the natural disorder of the universeS
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Spontaneous
thermodynamically possible, but it won't necessarily happen automatically
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Standard Gibbs Free energy formation
the free energy change that occurs when 1mol of elements is formed in standard state
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Gibbs Free Energy
the energy which is free to do useful work rather than just leave a system as heat
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Other cards in this set
Card 2
Front
the capacity or absorbing ability a system has for heat energy
Back
Heat capacity
Card 3
Front
the amount of energy that the given mass of a substance can absorb to produce 1C increase in temperature
Back
Card 4
Front
the change from chemical energy to heat energy
Back
Card 5
Front
The energy required to overcome the forces holding the particles together in a solid. Always endothermic.
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