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GCSE Chemistry > Unit 2b > Flashcards

Unit 2b Flashcards

1
Q

Rate of reaction =

A

Amount of reactant used / time
or
Amount of product formed / time

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2
Q

Activation energy

A

The minimum amount of energy particles must have to react

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3
Q

How can the rate of reaction be increased?

A

By increasing the temperature:
Increases the pressure of reactant gases
Increases the concentration of reactants in solutions
Increases the surface area of solid reactants

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4
Q

How does increasing the temperature increase the rate of reaction?

A

It increases the speed of the reacting particles so that they collide more frequently and more energetically

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5
Q

Catalyst

A

A substance which speeds up a reaction, without being changed or used up in it

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6
Q

Exothermic reaction

A

A reaction that transfers energy to the surroundings

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7
Q

Endothermic reaction

A

A reaction that takes in energy from the surroundings

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8
Q

If a reaction is exothermic in one direction, what reaction is it in the other direction?

A

Endothermic

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9
Q

All equation state symbols

A

(s), ( l ) , (g) and (aq)

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10
Q

(s) state symbol

A

Solid

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11
Q

(I) state symbol

A

Liquid

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12
Q

(g) state symbol

A

Gas

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13
Q

(aq) state symbol

A

Dissolved in water

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14
Q

Neutralisation reaction =

A

Acid + base -> salt + water

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15
Q

Neutralisation

A

A reaction between acids and alkalis

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16
Q

Acid + Base =

A

Salt + Water

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17
Q

Acid + Metal =

A

Salt + Hydrogen

18
Q

How can soluble salts be made?

A

Using a metal, alkali, or insoluble base

19
Q

How are insoluble salts made?

A

With a precipitation reaction

20
Q

What do electrolysis reactions involve?

A

Oxidation and reduction

21
Q

Electrolysis reaction mnemonic

A

OIL RIG

22
Q

OIL RIG

A

Oxidation Is Loss
Reduction Is Gain

23
Q

How can the rate of reaction be measured?

A

Precipitation
Change in mass
Volume of gas given off

24
Q

Precipitation

A

When the product of a reaction is a precipitate that clouds the solution

25
Q

Advantages of using catalysts in industrial processes

A

Reaction is quicker, so saves money
Allows the reaction to work at lower temperatures

26
Q

Disadvantages of using catalysts in industrial processes

A

Expensive
Different reactions need different catalysts
Catalysts can be poisoned by impurities, so they stop working

27
Q

Electrolysis

A

The breaking down of a substance with electricity

28
Q

Electroplating

A

Using electrolysis to coat the surface of one metal with another metal

29
Q

Uses of electroplating

A

Decoration
Conduction

30
Q

What are the products of the electrolysis of sodium chloride solution?

A

Hydrogen
Chlorine (Bleach)
Sodium hydroxide (Soap)

31
Q

Acid + Metal Oxide =

A

Salt + Water

32
Q

Acid + Metal Hydroxide =

A

Salt + Water

33
Q

Metal oxides and metal hydroxides =

A

Bases

34
Q

2HCl + Mg =
^ ^
(Acid) + (Metal)

A

MgCl2 + H2
^ ^
(Salt) + (Hydrogen)

35
Q

Negative electrode half equation

A

2_+ + 2e- –> _2

36
Q

Positive electrode half equation

A

2_- - 2e- –> _2

37
Q

How can you tell if a reaction is done at a high temperature?

A

If the product of a reaction is a gas

38
Q

Why are carbon nanotubes used as lubricants?

A

Because the layers can slide over each other as they don’t have covalent bonds between them

39
Q

Why can graphite conduct electricity?

A

It has free electrons so electrons can move through the graphite

40
Q

How can collecting and plotting more data improve the conclusions of an experiment?

A

You can reduce the effect of anomalous results

41
Q

How can a substance have a high melting point?

A

With strong bonds

GCSE Chemistry (5 decks)

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