Energy changes

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30 Terms

1
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What are the two types of energy changes ?

  • Exothermic

  • Endothermic

2
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What is an Exothermic reaction and state examples ?

  • A reactionf that transfers energy to its surrounding

  • The temperature of the surroundings increase

    Examples include

  • Combustion

  • Oxidation

  • Neutralisation

3
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What are the everyday uses of exothermic reactions ?

  • Self-heating cans

  • Hand warmers

4
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What is an endothermic reaction and what are some examples?

  • A reaction that takes in energy from the surroundings

  • The temperature of the surroundings decreases

    Examples include:

  • Thermal decomposition

  • The reaction of citric acid and sodium hydrogencarbonate

5
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What are the everyday uses of endothermic reactions?

  • Some sports injury packs are based on endothermic reaction

6
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What does the energy profile of an exothermic reaction look like?

ā€¢ Products have lower energy than reactants

ā€¢ Energy change for an exothermic reaction is negative

<p>ā€¢ Products have lower energy than reactants</p><p>ā€¢ Energy change for an exothermic reaction is negative</p>
7
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What is the activation energy ?

  • The minimum amount of energy that particles must have to react is called the activation energy

8
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How do we know a reaction is an exothermic reaction of the overall energy change is a negative number?

This is an exothermic reaction because the energy released from forming new bonds

is greater than the energy needed to break existing bonds.

9
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How do we know a reaction is an endothermic reaction of the overall energy change is a postive number?

This is an endothermic reaction as the energy needed to break existing bonds is

greater than the energy released from forming new bonds.

10
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How do cells produce chemicals?

  • Cells contain chemicals which react to produce electricity

11
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How can a simple cell be made?

ā€¢ A simple cell can be made by connecting two different metals in contact with an electrolyte.

ā€¢ The two electrodes are metals as they conduct electricity delocalised electrons which carry electrical charge.

ā€¢ The electrolyte is a solution that conducts electricity and contains ions which are free to move and carry electrical charge.

12
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How can batteries produce a greater voltage?

  • Two or more cells connected in series produce a larger voltage

13
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What is the voltage produced by the cell dependent on?

  • Type of electrode

  • Type of electrolyte

14
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In non rechargeable batteries when does it stop working?

  • When one of the reactants been used up

15
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Are alkaline batteries rechargeable or non rechargeable?

  • Non rechargeable

16
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If there is a larger difference in reactivity, what does this tell us about the voltage ?

  • Greater voltage

17
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What type of ions do alkaline batteries include and what are the uses of this battery?

  • OH- ions (hydroxide ions)

  • Used in remote controls

18
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Why can rechargeable batteries recharge?

  • Rechargeable cells and batteries can be recharged because the chemical reactions are reversed when an external electrical current is supplied.

19
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What are the difference between the processes in electrolysis and in a chemical cell?

o Electrolysis uses electricity to produce a chemical reaction

o Cells use a chemical reaction to produce electricity

20
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When will the voltage be zero in a cell?

ā€¢ The electrodes are made of the same metal

ā€¢ The reactivity of the metals is the same

21
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What is a fuel cell?

  • Fuel cells are supplied by an external source of fuel (eg hydrogen) and oxygen or air.

  • The fuel is oxidised electrochemically within the fuel cell to produce a potential difference.

22
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What does the overall reaction in a hydrogen fuel cell involve ?

ā€¢ The overall reaction in a hydrogen fuel cell involves the oxidation of hydrogen to produce water.

23
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How do fuel cells produce electricity?

  • Fuel and oxygen to produce electrical energy

24
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How do hydrogen-oxygen fuel cells work?

ā€¢ Electrolyte is often a solution of phosphoric acid and the electrodes are often porous carbon with a catalyst

ā€¢ Hydrogen gas goes into the anode and oxygen into the cathode

ā€¢ At the anode the hydrogen loses electrons to form hydrogen ions

ā€¢ Hydrogen ions in the electrolyte moves to the cathode

ā€¢ At the cathode, oxygen gains electrons from the cathode and reacts with hydrogen ions to make water

ā€¢ The electrons flow through an external circuit from the anode to the cathode. This is the electric current.

25
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What are the products of a hydrogen-oxygen fuel cell?

  • Water and energy

26
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As hydrogen-oxygen fuel cells involve a redox reaction what occurs at the anode and cathode + half equations?

  • Anode - Oxidation

  • Hydrogen loses electrons to form hydrogen ions

    H2 ā†’ 2H+ + 2e-

  • Cathode - Reduction

  • Oxygen gains electrons from the cathode and reacts with hydrogen ions to make water

    O2 + 4H+ 4e- ā†’ 2H2O

27
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What is the overall equation for a hydrogen-oxygen fuel cell?

knowt flashcard image
28
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What are the advantages and disadvantages of Hydrogen fuel cells?

Hydrogen Fuel cells

Advantages

ā€¢ No pollutants-Produces only water

ā€¢ Do not need recharging

ā€¢ Hydrogen can be made renewable if made by electrolysis using renewable energy.

Disadvantages

ā€¢ Hydrogen is highly flammable

ā€¢ Hydrogen is difficult to store/takes up a lot of space

ā€¢ Hydrogen not renewable if produced using fossil fuels

ā€¢ Not many hydrogen filling stations

29
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What are the advantages and disadvantages of rechargeable batteries?

Rechargeable batteries

Advantages

ā€¢ Charging points more widely available

ā€¢ Rechargable

Disadvantages

ā€¢ May release toxic chemicals on disposal

ā€¢ Rechargeable batteries have finite life-time

ā€¢ Can catch fire

ā€¢ Store less energy than fuel cells

30
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What is a potential alternative to rechargeable batteries and cells?

Hydrogen fuel cells