Ch. 5: Chemical Kinetics Flashcards

1
Q

What is the relationship between the variables in the Arrhenius equation?

A

Arrhenius Equation: k=Ae^(-Ea/RT)
k is the rate constant

As T ↑ k ↑
As Ea ↑ k ↓

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2
Q

What does the variable A in the Arrhenius equation represent? How does it change?

A

A is the frequency factor of collisions. It is increased by increasing the concentration of molecules, which increases the number of collisions.

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3
Q

What are four factors that affect reaction rate?

A

Reaction concentrations
Temperature
Medium of reaction
Catalysts

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4
Q

Increasing the reaction concentration increases the reaction rate for all EXCEPT what type of reaction?

A

Zero-order reactions because their rate does not depend on the concentration of reactants.

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5
Q

Why does increasing temperature increase reaction rate?

A

As temperature increases, the average kinetic energy of molecules increases. Therefore, reactants gain more energy to surpass Ea.

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6
Q

What is the difference between homogenous and heterogeneous catalysis?

A

Homogenous catalysis: catalyst is in the same phase (solid, liquid, gas) as reactants.

Heterogenous catalysis: catalyst is in a different phase compared to reactants.

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7
Q

What is the rate law of a zero-order reaction?

A

rate = k

The rate of formation of the product is INDEPENDENT of changes in concentration of reactions.

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8
Q

What are the units of k in a zero-order reaction?

A

M/s

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9
Q

What factors change the rate of a zero-order reaction?

A

Temperature

Catalyst: lowers Ea and increases k

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10
Q

What is the concentration vs time equation of a zero-order reaction? What does this look like on a graph?

A

[A] = [A]o - kt

Graph: negative linear with slope = -k

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11
Q

What is the rate law of a first-order reaction?

A

rate = k[A]^1

The rate is directly proportional to only ONE reactant.

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12
Q

What are the units of k in a first-order reaction?

A

1/s = s^-1

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13
Q

What is a classic example of a first-order reaction?

A

Radioactive decay — the reactant undergoes a chemical change all by itself, without chemical or physical interaction with another molecule

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14
Q

What is the integrated rate law of first-order reaction? what does the graph look like?

A

[A] = [A]o e^(kt)
ln [A] = ln[A]o - kt
The graph of ln [A] = ln[A]o - kt is negative linear with a slope = -k

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15
Q

What is the rate law of a second-order reaction?

A
rate = k[A]^2  or
rate = k[B]^2  or
rate = k[A]^1 [B]^1
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16
Q

What are the units of k in a second-order reaction?

A

1/Ms

17
Q

What is the integrated rate law of second-order reaction? what does the graph look like?

A

1/[A] = 1/[A]o + kt

The graph looks positive linear with slope = k