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Energetics > Definitions > Flashcards

Definitions Flashcards

1
Q

enthalpy change

A

when 1 mole of covalent bonds, in a gaseous molecule, is broken under standard conditions

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2
Q

Endothermic

A

absorbs heat energy into the system

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3
Q

Exothermic

A

releases heat energy from the system

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4
Q

Heat

A

form of energy that flows from high to low temperature

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5
Q

Temperature

A

measure of the average kinetic energy of particles in a substance

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6
Q

specific heat capacity of water

A

4.18

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7
Q

heat energy formula

A

q=mc(Tf-Ti)

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8
Q

enthalpy change formula

A

H= (mc(Tf-Ti)) / n

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9
Q

enthalpy change of formation

A

enthalpy change when 1 mole of a substance is formed from its elements in their standard states under standard conditions

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10
Q

enthalpy change of diatomic atoms

A

0

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11
Q

lattice energy

A

enthalpy change when 1 mole of a crystal lattice is turned into its infinitely separated gaseous ions under standard conditions

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12
Q

born-haber cycle

A

enthalpy level of diagram breaking down the formation of an ionic compound into a series of simpler steps

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13
Q

enthalpy change of solution

A

enthalpy change when 1 mole of solute is dissolved in excess solvent to form a solution of infinite dilution under standard conditions

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14
Q

enthalpy change of hydration

A

enthalpy change when 1 mole of gaseous ions is surround by water molecules to form an infinitely dilute solution under standard conditions

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15
Q

entropy

A

how available energy is distributed among particles

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16
Q

gibbs free energy

A

to see whether reaction is spontaneous or not

17
Q

enthalpy change of neutralisation

A

enthalpy change when 1 mole of water molecules are formed when an acid (H+) reacts with an alkali (OH-) under standard conditions

18
Q

spontaneous reactions

A

a reaction that occurs without any outside influence

19
Q

average bond enthalpy

A

average amount of energy required to break 1 mole of a gaseous molecule

Energetics (1 decks)

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