3.1.4 Energetics

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Total cards: 24•Content version: v3•Public deck•Updated: 8/1/2026

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Front (Question)

how is enthalpy change represented

Back (Answer)

delta H

Front (Question)

define enthalpy change

Back (Answer)

heat energy transferred in a reaction at constant pressure

Front (Question)

units for enthalpy change

Back (Answer)

kJ mol-1

Front (Question)

what does delta H with the tube symbol mean

Back (Answer)

the reactants and products where in there standard states and that the measurements were made under standard conditions

Front (Question)

what are standard conditions

Back (Answer)

100kPa (around 1atm) pressure and a stated temperature

Front (Question)

what is a common stated temperature used

Back (Answer)

298K / 25 degrees Celsius

Front (Question)

what does it mean if enthalpy change includes an r

Back (Answer)

enthalpy change is for a reaction

Front (Question)

what does it mean if enthalpy change includes a c

Back (Answer)

enthalpy change is for combustion

Front (Question)

what does it mean if enthalpy change includes an f

Back (Answer)

enthalpy change is for formation of a new compound

#10

Front (Question)

exothermic reactions

Back (Answer)

give out energy to their surroundings so temperature in the reaction usually goes up

#11

Front (Question)

enthalpy change for exothermic reactions

Back (Answer)

delta H value is negative

#12

Front (Question)

why is the delta H value for exothermic reactions negative

Back (Answer)

products of the reaction end up with less energy than the reactants

#13

Front (Question)

is oxidation usually exothermic or endothermic

Back (Answer)

exothermic

#14

Front (Question)

endothermic reactions

Back (Answer)

endothermic reactions take in energy from their surroundings, so the temperature in the reaction usually falls

#15

Front (Question)

enthalpy change for endothermic reactions

Back (Answer)

delta H is positive

#16

Front (Question)

why is delta H value for endothermic reactions positive

Back (Answer)

products of the reaction have more energy than the reactants

#17

Front (Question)

what are bond enthalpies

Back (Answer)

bond enthalpy is the energy needed to break a bond

#18

Front (Question)

is bond breaking exothermic or endothermic

Back (Answer)

bond breaking is endothermic as you need energy to break bonds

#19

Front (Question)

is bond making exothermic or endothermic

Back (Answer)

bond making is exothermic as energy is released when bonds are formed

#20

Front (Question)

does energy required to break a certain bond change

Back (Answer)

energy required to break a certain type of bond can change depending on where it is

#21

Front (Question)

what avg do you use for bond enthalpies in calculations

Back (Answer)

in calculations you use mean bond enthalpy

#22

Front (Question)

what is mean bond enthalpy

Back (Answer)

average energy needed to break a certain type of bond, over a range of compounds

#23

Front (Question)

when is energy absorbed (in bonds)

Back (Answer)

energy is absorbed to break bonds

#24

Front (Question)

when is energy released (in bonds)

Back (Answer)

energy is released to form bonds