Physical Chapter 5: Kinetics, Equilibria, and Redox Flashcards

1
Q

What is reaction rate defined as?

A

The amount of reactant used or product formed over time

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2
Q

What is Collision theory?

A

The idea that particles have to collide with a sufficient amount of kinetic energy in order to react

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3
Q

What is Activation energy?

A

The minimum amount of energy needed for particles to react

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4
Q

What is the Maxwell-Boltsman distribution?

A

A graph showing the distribution of molecules at certain energy levels

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5
Q

What does the area under the Maxwell-Boltsman curve represent?

A

The total number of molecules

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6
Q

What is the effect of increasing temperature on reaction rate?

A

Rate will increase

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7
Q

Why does increasing temperature increase rate of reaction?

A

Each molecule will have greater energy and therefore more will meet the activation energy.

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8
Q

What is the effect of increased concentration on rate of reaction?

A

It will increase the rate

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9
Q

What is the effect of increased pressure on rate of reaction?

A

It will increase the rate

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10
Q

What is the effect of a catalyst on rate of reaction?

A

It provides an alternate pathway for the reaction with a loer activation energy - rate will increase

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11
Q

What are the three main ways to measure reaction rates?

A

Time taken for a precipitate to form
Measuring a decrease in mass
Measuring volume of gas given off

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12
Q

What is a reversible reaction?

A

A reaction that can go either way

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13
Q

What is dynamic equilibrium?

A

All products and reactants’ concentrations stay constant

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14
Q

What is Le Chatelier’s principle?

A

If a reaction at equilibirum is subjected to a change, the position of equilibrium will move to counter that change.

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14
Q

What is Le Chatelier’s principle?

A

If a reaction at equilibirum is subjected to a change, the position of equilibrium will move to counter that change.

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14
Q

What is Le Chatelier’s principle?

A

If a reaction at equilibirum is subjected to a change, the position of equilibrium will move to counter that change.

15
Q

What will happen if you increase the temperature of an equilibrium mixture?

A

The position of Equilibrium will move in the endothermic direction

16
Q

What will happen if you increase the concentration of a product in an equilibrium mixture?

A

The position of equilibrium will move to the left to produce more reactant

17
Q

What will happen if you increase the pressure of an equilbrium mixture?

A

The position of equilbrium will move towards the side with less molecules

18
Q

What effect do catalysts have on position of equilibrium?

A

None

19
Q

What affects how reaction conditions are chosen in industry?

A

Compromise between speed, yield, and cost of production

20
Q

What is the Equilibrium constant written as?

A

Kc

21
Q

What is the formula for Kc?

A

Where aA + bB <-> cC + dD,
Kc = [D]d[C]c/[A]a[B]b

22
Q

What is the only factor that affects Kc?

A

Temperature

23
Q

How does temperature affect Kc?

A

If it means there is more product at equilibrium, Kc will rise. If it means less product at Equilibrium, Kc will fall.

24
Q

What is the definition of a redox reaction?

A

Any reaction where electrons are transferred

25
Q

What is oxidation?

A

Loss of electrons

26
Q

What is reduction?

A

Gain of electrons

27
Q

What is an oxidising agent?

A

A chemical that gets reduced

28
Q

What is a reducing agent?

A

A chemical that gets oxidised

29
Q

How do you assign oxidation states?

A

Overall oxidation state is equal to the charge of the ion or compound
Oxidation state of each element is often the same as the charge on its ion (e.g. O will often be 2-)

30
Q

How do you combine half-equations?

A

Make sure the charges & electrons match