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Chemistry C2 > C2 Rates of Reaction > Flashcards

C2 Rates of Reaction Flashcards

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1
Q

What effect will increasing the temperature have on the rate of reaction?

A

Increase

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2
Q

What effect will decreasing the concentration of a solution have on the rate of reaction?

A

Decrease

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3
Q

What effect will using smaller pieces of solid have on the rate of reaction?

A

Increase

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4
Q

What will happen to the rate of reaction if the temperature is decreased?

A

Decrease

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5
Q

How does changing the surface area of a solid affect the rate of a reaction?

A

Increasing the surface area will increase the rate of reaction

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6
Q

How do you increase the surface area of a solid?

A

Break it up into smaller pieces

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7
Q

What do atoms need to do to react?

A

Collide with enough force

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8
Q

Why does increasing the temperature increase the rate of reaction?

A

Increasing the temperature gives the particles more energy, so they move faster. This means - they collide more often - they collide with more force

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9
Q

Why does increasing the concentration increase the rate of reaction?

A

A higher concentration means there are more particles present, so they are more likely to collide.

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10
Q

Why does increasing the surface area increase the rate of reaction?

A

More particles are available to react, so the number of collisions increases.

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11
Q

What effect does a catalyst have on the rate of reaction?

A

Increases the rate of reaction.

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12
Q

Why does a catalyst increase the rate of reaction?

A

It provides an alternative pathway that requires less activation energy.

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13
Q

How does increasing the pressure affect the rate of reaction?

A

Increases

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14
Q

Why does increasing the pressure increase the rate of reaction?

A

The particles are closer together therefore collide more often.

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15
Q

What are the different ways we can measure the rate of a reaction?

A
  1. Measure the time taken for a reactant to be used up. 2. Measure the volume of gas produced. 3. Measure the decrease in mass (if a gas is produced). 4. Measure the time taken for a cross to no longer be visible (if a solid is produced).
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16
Q

Which would react faster - a reaction at 50 degrees C or one at 80 degrees C?

A

80 degrees

17
Q

Which would react faster - a reaction using 2.0M acid or one using 1.5M?

A

2.0M

18
Q

Which would react faster, 2g of powdered limestone or limestone chips?

A

Powdered limestone

19
Q

Give some advantages of using catalysts.

A

Reaction can be carried out at lower temperature so saves money and less pollution made Product can be made at a faster rate Catalyst does not get used up in the reaction

20
Q

Give some disadvantages of using catalysts

A

Often very expensive Can be poisonous to the environment Different catalysts are needed for different reactions

21
Q

What is a catalyst?

A

Something that speeds up the rate of a reaction without being used up.

22
Q

What happens in an exothermic reaction?

A

Energy is released as heat and the temperature goes up.

23
Q

What happens in an endothermic reaction?

A

Energy is taken in and the temperature goes down.

24
Q

A reaction is carried out between zinc metal and copper sulfate. The temperature increases during the reaction. Is it exothermic or endothermic?

A

Exothermic - the temperature goes up.

25
Q

Some ammonium chloride is dissolved in water which decreases the temperature of the water. Is this an exothermic or endothermic change?

A

Endothermic - the temperature goes down.

26
Q

Give an example of an endothermic reaction

A

Photosynthesis Thermal decomposition

27
Q

Give an example of an exothermic reaction

A

Respiration Combustion

28
Q

How can exothermic reactions be useful?

A

Heat packs Self-heating drinks

29
Q

How can endothermic reactions be useful?

A

Cold packs

30
Q

What is a reversible reaction?

A

As soon as the products are made they react together to form the reactants. The reaction can go backwards and forwards.

31
Q

What does this symbol mean?

A

Reversible reaction

Chemistry C2 (5 decks)

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