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Chemistry 12 > Equilibrium > Flashcards

Equilibrium Flashcards

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1
Q

Rate of reaction is measured in _________

A

Moles per litre per second

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2
Q

What does the kinetic molecular theory state?

A
  • all matter is made up of microscopic sized particles.
  • particles are in constant motion because they possess kinetic energy.
  • there are spaces between the particles of matter. The speed and spacing determine the physical state of matter.
    Adding heat increases the speed of moving particles therefore increasing their kinetic energy as well as the space they occupy.
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3
Q

What does the collision theory state?

A

In order for a reaction to occur, reacting particles must collide successfully with one another.

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4
Q

Increasing the temperature of a reaction results in an increase of decrease of reaction rate?

A

Increase.

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5
Q

Reactions that involve breaking fewer bonds are generally faster or slower than reactions that involve breaking a greater number of bonds?

A

Faster.

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6
Q

Reactions that involve breaking stronger bonds are generally faster or slower than reaction that involve breaker stronger bonds?

A

Slower.

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7
Q

Are reactions that involve ionic compounds and simple ions generally faster or slower than reactions involving molecular compounds?

A

Faster.

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8
Q

The change in the amount of reactants or products over time is called the ___________

A

Reaction rate or rate of reaction

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9
Q

What are the five factors that affect reaction rate?

A
  1. Temperature
  2. Concentration
  3. Surface area
  4. Catalyst
  5. Reactivity of the recants
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10
Q

Fora collisions between reactants to result in a collision, the collision must satisfy which two criteria?

A
  1. Correct orientation of reactant particles

2. Sufficient collision energy

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11
Q

What is refers to as the top of the “hill” on a potential energy diagram?

A

Transition state.

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12
Q

What is the activated complex?

A
  • a transitional species that exists for a fraction of a moment and is neither product nor reactant.
  • it has partial bonds and is highly unstable
  • the chemical species that exists at the transition point
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13
Q

What is a reaction mechanism?

How does if differ from the elementary reaction?

A

A series of steps that make up an overall reaction. Each step that involves absinthe molecular event is called an elementary reaction.

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14
Q

What are molecules that are formed in an elementary reaction and consumed in a subsequent reaction?

A

Reaction intermediates.

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15
Q

How many particles collide and react when the elementary reaction is said to be unimolecular, bimolecular, and termecular respectively?

A

One, two, and three.

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16
Q

Are reaction mechanisms proposed or stated?

A

Proposed because it only appears for a short time.

17
Q

What step is the rate-determining step?

A

One elementary reaction that is much slower that determines the overall rate.

18
Q

What is a catalyst?

A

A substance that increases the rate of a chemical reaction without being consumed by the reaction.

19
Q

How does a catalyst work?

A
  • It works by lowering the activation energy of a reaction so that a larger fraction of the reactants have sufficient energy to react.
  • It lowers the activation energy by providing an alternate mechanism for the reaction.
20
Q

What is the difference between a homogeneous catalyst and a heterogeneous catalyst?

A

Homogeneous- exists in the same phase as the reactants.

Heterogeneous- exists in a phase that is different from the phase of the reaction it catalysts.

21
Q

What are the 4 equilibrium conditions?

A
  1. It is achieved in a reversible process when the rates of opposing charges are equal.
  2. The observable (macroscopic) properties of a system at equilibrium are constant. (Ex, colour, pressure, concentration, and pH)
  3. It can only be reached in a closed system.
  4. It can be approached from either direction.
22
Q

What is the law of chemical equilibrium?

A

At equilibrium, there is a constant ratio between the concentrations of the products and reactants in any change.

23
Q

What is the equilibrium constant?

A

For any chemical reaction at equilibrium and at a given temperature there is a specific ratio of concentration terms.

24
Q

What does ICE table stand for?

A

Initial
Change
Equilibrium

25
Q

When K > 1, what is favoured?

A

Products.

26
Q

When K

A

Reactants.

27
Q

When K = 1, what is favoured?

A

There are approximately equal concentration of reactants and products at equilibrium.

28
Q

Are solids accounted for in an ICE table?

A

No. It is not included.

29
Q

If your initial concentration divided by the value of Kc is greater than what number, what can be justified?

A

If it is greater than 500, approximation is justified in a way that you do not need to account for a change in concentration for the reactants.

30
Q

If Qc > Kc, which what does it shift?

A

Towards reactants.

31
Q

If Qc

A

Towards products.

32
Q

If Qc = Kc, which what does it shift?

A

It is at equilibrium.

33
Q

That is the reaction quotient? (Qc)

A

It is an expression that is identical to the equilibrium constant expression, but its value is calculated using concentrations that are not necessarily those at equilibrium.

34
Q

What is Le Châtelier’s Principle?

A

A dynamic equilibrium tends to respond so as to relieve the effect of any change in the conditions that affect the equilibrium.

35
Q

Does a catalyst affect equilibrium?

A

It speeds up the rate of a reaction. It does not affect the position of equilibrium, only the time that is taken to achieve equilibrium.

36
Q

If you increase temperature, does it favour an exothermic or endothermic direction?

A

Endothermic.

37
Q

What does the common ion effect do ti a system?

A

Equilibrium shifts away from the added ion.

38
Q

Do strong or weaker acids in a reaction make it go faster?

A

Stronger acids will occur faster.

Chemistry 12 (5 decks)

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