Chapter 5 Flashcards

1
Q

Combination Reaction

A

Two molecules come together to form an intermediate that decomposes to produce two final products

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2
Q

Rate-determining Step

A

Slowest step of a reaction
* Determines overall rate of reaction
* Reaction can only proceed as fast as rate-determining step

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3
Q

Activation Energy

A

Minimum energy needed for a chemical reaction to occur
* Distance on y-axis from energy of reactants to peak energy before formation of products
* Lowest activation energy = fastest rate of reaction

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4
Q

Transition State Theory

A

Focuses on forming high-energy activated complex that can then proceed forward/backward, forming products or reverting to reactants

  • Requires certain activation energy to be overcome for a reaction to occur
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5
Q

Collision Theory

A

Focuses on energy and orientation of reactants and considers each potential reaction to be all-or-nothing (either enough energy to form products or not)

  • Requires certain activation energy to be overcome for a reaction to occur
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6
Q

Zero-Order Reaction

A

Have constant rate that doesn’t depend on concentation of reactant

  • Temperature lowered: rate decreased
  • All reactants’ concentrations doubled: rate unaffected
  • Catlyst added: rate increased
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7
Q

First-Order Reaction

A

Has a nonconstant rate that depends on concentration of reactant
* Temperature lowered: rate decreased
* All reactants’ concentrations doubled: rate doubled
* Catalyst added: rate increased

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8
Q

Second-Order Reaction

A

Has nonconstant rate that depends on concentration of reactant
* Temperature lowered: rate decreased
* All reactants’ concentrations doubled: rate multiplied by 4
* Catalyst added: rate increased

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9
Q

Endothermic

A
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10
Q

Exothermic

A
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11
Q

Spontaneous Reaction (Exergonic)

A

Net free energy change is negative

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12
Q

Nonspotaneous (Endergonic) Reaction

A

Net free energy change is positive

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13
Q

Rate of Reaction

A
  • Temperature directly affects rate constant
  • Changing partial pressure of gas will affect number of effective collisions per time
  • Solvents affect rate of reactions depending on reaction solvent interaction
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14
Q

Saturated Catalyst

A
  • Have maximum turnover rate
  • Can’t increase rate constant or reaction rate any higher by adding more reactant
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15
Q

Catalyst

A

Increases the rate of reaction by lowering the activation energy making it easier for both forward and reverse reactions to overcome energy barrier
* Not used up
* Don’t alter equilibrium of reaction
* Stabilize transition state by lowering energy, not raising or eliminating

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