Chemical Kinetics Flashcards

1
Q

Arrhenius equation

A

k = Ae^-(Ea/RT)

  • A = freq collisions, coef
  • Ea: activaiotn energy
  • R: ideal gas constant
  • T: temp (K)
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2
Q

What are the two factors influence rate constant? and how?

A

Ea: activation energy, inversely proportional
T: directly proportional

Lower activation energy, increases rate constant
Incr temp: incr rate constant

Ea: more frequently manipulated

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3
Q

0 Order vs 1st Order

A

M/S vs 1/S

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4
Q

Endo vs Exothermic

A

Endothermic: delta H > 0
- products more energy than reactants

Exothermic: delta H <0
- reactants more than products

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5
Q

Units of rate

A

Molarity/Sec

- units of molarity are Mol/Liter

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6
Q

What is the overall rate order of a rate equation?

A

add up exponents

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7
Q

True or false: rate order can be determined with stoichometry

A

false: need to test experimentally as well

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8
Q

What are common 0 order reactions

A
  • radioactive decay and SN1
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9
Q

what are common 2nd order reations

A
  • collission and SN2
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10
Q

Formula for Kcat

A

Vmax / E total

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11
Q

Formula for catalytic efficiency

A

Kcat / km

  • Kcat = Vmax / E total
  • Vmax = k cat * E total
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