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Topic: Potential Energy Curve Do Now : p.26. Spontaneous Processes. =physical or chemical change that occurs with no outside intervention However, some energy may be supplied to get process started = activation energy. Iron rusting 4Fe(s) + 3O 2 (g)  2Fe 2 O 3 (s)  H = -1625 kJ.

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spontaneous processes
Spontaneous Processes

=physical or chemical change that occurs with no outside intervention

  • However, some energy may be supplied to get process started = activation energy

Iron rusting

4Fe(s) + 3O2(g)  2Fe2O3(s)

H = -1625 kJ

CombustionCH4(g) + 2O2(g)  CO2(g)+ 2H2O(l)

H = -891kJ

activation energy
Activation Energy
  • = Energy needed to initiate reaction
  • Energy needed to overcome reaction barrier
  • difference between where reactants start & top of hill
  • Difference between reactants & activated complex
energy diagram of a reaction

Activated Complex = intermediate

formed during conversion from reactants to products

Reactants combine to form an unstable complex

Energy Diagram of a Reaction
potential energy curve endothermic
Potential Energy Curve: Endothermic

Products have more P.E. than reactants

Start low, end high

potential energy curve exothermic
Potential Energy Curve: Exothermic

Products have less P.E. than reactants

Start high, end low

have to label 6 energies on curve reactants products
Have to label 6 energies on curve: reactants & products
  • PE reactants
  • PE products
  • PE activated complex
  • Ea forward reaction
  • Ea reverse reaction
  • H
slide12

PE

reactants

Time

What kind of reaction is represented?

40

Ea

reverse rxn

Ea

forward rxn

30

Enthalpy 

20

PE activated complex

PE products

10

slide13

40

30

Enthalpy 

H of reaction

20

10

slide14

Ea

forward

rxn

Ea

reverse

rxn

40

30

Enthalpy 

PE of activated complex

20

PE of reactants

10

P.E. of products

Time

What kind of reaction is represented?

slide15

40

30

Enthalpy 

20

H of reaction

10

catalyst in the body enzyme
Catalyst (in the body = enzyme)
  • Substance that increases rate of reaction without itself being consumed
    • does not participate in reaction
  • Lowers the activation energy for the reaction
slide17

DOES IT AFFECT ΔH?

Catalysts do not affect ΔH

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