14-3 Flashcards

1
Q

Activation energy on a graph equals

A

-Slope * R (R is a constant = 8.314)

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2
Q

For the reaction to proceed, the energy barrier (activation energy)

A

must be “crossed”. At the highest energy state, the transition state (activated complex) is formed.​

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3
Q

Activation energy is the energy needed to form (reach)

A

the transition state.​
Transition state is not a stable species. It lasts shorter time than one vibration. ​

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4
Q

Another factor to consider, which affects the rate​ is the…

A

Orientation of molecules (14.3-pg.8)

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5
Q

There is a big difference between the transition state and the intermediate. What is it?

A

transition states are not stable species. ​
Intermediates are stable. In some instances, it is possible to isolate an intermediate.​

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6
Q

Catalysts increase the rate of a reaction…

A

without being used up themselves, by decreasing the activation energy of the reaction.​

Catalysts do this by changing the mechanism by which the process occurs (more elementary steps, but with smaller activation energies).​

Catalyst reacts in one step and is regenerated in another step, so it does not appear in the net equation.​

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7
Q

Type of catalysts are…

A

Homogeneous catalysts​
Heterogeneous catalysts​
Enzymes – Nature’s Catalysts​

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8
Q

Homogeneous Catalysts​ are

A

The reactants and catalyst are in the same phase.​

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9
Q

Heterogeneous Catalysts​ are

A

The catalyst is in a different phase than the reactants.​
Often, gases are passed over a solid catalyst.
The adsorption of the gas molecules of the reactants on the surface of a solid catalyst is often the rate-determining step.​​

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10
Q

Enzymes​ are

A

biological catalysts
Enzymes are very specific. ​
The substrate fits into the active site of an enzyme, much like a key fits into a lock.​

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