Chapter 10 - Reaction Rates and Equilibrium Flashcards

Reaction rates, Catalysts, Boltzmann distribution, Dynamic equilibrium and le Chatelier's principle, and The equilibrium constant.

1
Q

What is reaction rate?

A

The change in concentration of a reactant or product in a given time.

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2
Q

What makes an effective collision?

A

Particles must have sufficient energy

Particles must collide in correct orientation

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3
Q

Which factors can change the rate of a chemical reaction?

A

Concentration

Temperature

Use of a catalyst

Surface area of solid reactants

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4
Q

What effect does increasing temperature have on reaction rate?

A

Reaction rate increases

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5
Q

Explain why increasing temperature has its effect on reaction rate

A

Particles have more energy

Higher speed

Collide more frequently

More successful collisions

Rate increases

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6
Q

What is the rule of thumb for reaction rate and temperature?

A

A 10C increase in temperature doubles the rate.

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7
Q

What effect does increasing concentration/pressure have on reaction rate?

A

Reaction rate increases

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8
Q

Explain why increasing concentration/pressure has its effect on reaction rate

A

Concentration increases

More particles per unit volume

More frequent collisions

More successful collisions

Rate increases

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9
Q

How can progress of a chemical reaction be followed?

A

Monitoring the removal of a reactant.

Following the formation of a product.

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10
Q

What are the two methods of determining reaction rate, when a gas is produced?

A

Monitoring the volume of gas produced

Monitoring the loss of mass of reactants

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11
Q

What does a catalyst do?

A

A substance that changes the rate of a chemical reaction without undergoing any permanent change itself.

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12
Q

What are the main properties of a catalyst?

A

Not used up in the reaction.

May react with a reactant to form an intermediate or provide a surface for the reaction to take place.

The catalyst is regenerated at the end of the reaction.

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13
Q

What is a homogeneous catalyst?

A

Has the same physical state as the reactants.

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14
Q

How does a homogeneous catalyst interact with the reactants?

A

The catalyst reacts with the reactants to form an intermediate.

The intermediate then breaks down to give the product and regenerates the catalyst

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15
Q

Give two examples of homogeneous catalysts

A

Sulphuric acid in the production of esters

Chlorine radicals in ozone depletion

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16
Q

What is a heterogeneous catalyst?

A

Has a different physical state from the reactants.

17
Q

How does a heterogeneous catalyst interact with the reactants?

A

Heterogeneous catalysts are usually solids in contact with gaseous reactants or reactants in solution.

Reactant molecules are adsorbed (weakly bonded) onto the surface of the catalyst, where the reaction takes place.

After the reaction, the products leave the surface of the catalyst by desorption.

18
Q

Give examples of heterogeneous catalysts

A

Iron in making ammonia

Platinum or rhodium in reforming Nickel in hydrogenation of alkenes

Vanadium oxide in the making sulfur trioxide

19
Q

What are the benefits of using a catalyst?

A

Lowers activation energy

Less electricity used

Product made faster and cuts costs and increases profit

Less fossil fuels used cuts emissions of carbon dioxide

20
Q

What are the main features of Boltzmann distribution?

A

No molecules have zero energy

Area under the curve is equal to the number of molecules

No maximum energy

21
Q

How does a Boltzmann distribution curve change when temperature is increased?

A

The peak is lower and shifted to the right

A greater proportion of molecules can overcome the activation energy

22
Q

How does a Boltzmann distribution show the effect of a catalyst?

A

Activation energy with a catalyst is lower than normal activation energy.

Therefore a greater proportion of molecules exceed the new lower activation energy.

23
Q

What is a dynamic equilibrium?

A

The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and concentrations do not change.

24
Q

What is le Chatelier’s principle?

A

When a system in dynamic equilibrium is subjected to an external change, the system readjusts itself to minimise the effect of that change.

25
Q

What is the effect of a catalyst on equilibrium?

A

Does not change the position

Speeds up the rates of forward and reverse reactions equally

26
Q

If a reversible reaction is shown as: aA + bB cC + dD how is Kc worked out?

A

Kc = [C]^c x [D]^d / [A]^a x [B]^b

27
Q
A