Separate Chemistry - 5.5 Flashcards

1
Q

Name the following reactions that:

a) Take in heat from the surroundings
b) Give out heat to the surroundings

A

a) Endothermic
b) Exothermic

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2
Q

Name the type of reaction used in self-heating cups and hand warmers.

A

Exothermic reaction

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3
Q

Give an example of a chemical reaction that is exothermic.

A

Examples include: Combustion, Oxidation, Neutralisation

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4
Q

How do you know the reaction profile below is for an exothermic reaction?

A

Energy of products is lower than the energy of reactants

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5
Q

What can be said about the amount of energy before a chemical reaction and the amount of energy after a chemical reaction?

A

They are equal

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6
Q

Give an example of a chemical reaction that is endothermic.

A

Examples include: Thermal Decomposition and Reacting Citric Acid with Sodium hydrogencarbonate

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7
Q

Name the type of reaction is used in sports injury packs.

A

Endothermic reaction

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8
Q

How do you know the reaction profile below is for an endothermic reaction?

A

Energy of products is higher than the energy of reactants

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9
Q

Draw an energy level diagram (reaction profile) for an exothermic reaction.

A
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10
Q

What is the name for the minimum amount of energy needed for a reaction to happen?

A

Activation energy

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11
Q

Higher Q. Complete the sentences:

In a chemical reaction:

a) Energy is needed to ……………….
b) Energy is released when ……….

A

a) Energy is needed to break bonds
b) Energy is released when bonds are formed

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12
Q

Calculate the overall energy change in this reaction.

Bond energies: NN = 941 kJ/mol ; N-H = 391 kJ/mol ; H-H = 436 kJ/mol

*this is just an example, you may have to do this for any reaction. You will be given the bond energies.

A

Reactants: (6 x 391) = 2346

Products: (1 x 941) + (3 x 436) = 2249

2346 – 2249 = + 97 kJ/mol

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13
Q

Draw an energy level diagram (reaction profile) for an endothermic reaction.

A
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14
Q

Look at the reaction profiles below. Which arrows show the activation energy and which arrows show the overall energy change?

A
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15
Q

Higher Q. Calculate the overall energy change in this reaction.

Bond energies: C-H = 413 kJ/mol ; O=O = 495 kJ/mol ; C=O = 799 kJ/mol ; H-O = 463 kJ/mol

*this is just an example, you may have to do this for any reaction. You will be given the bond energies.

A

Reactants: (4 x 413) + (2 x 495) = 2642

Products: (2 x 799) + (4 x 463) = 3450

2642 – 3450 = -808 kJ/mol

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16
Q

Higher Q. Explain, in terms of bonds and energy, what makes a reaction…

a) … exothermic.
b) … endothermic

A

a) Exothermic: The energy released from forming new bonds is greater than the energy needed to break existing bonds.
b) Endothermic: The energy needed to break existing bonds is greater than the energy released when new bonds are formed.

17
Q

Separate Q. Suggest a factor that can affect the voltage produced by a cell.

A

Factors include: Type of electrode , Type of electrolyte

18
Q

Separate Q. Describe how to make a simple cell.

A

Connecting two different metals in contact with an electrolyte.

19
Q

Separate Q. What is a battery?

A

Two or more cells connected in series

20
Q

Separate Q. Are alkaline batteries rechargeable or non-rechargeable?

A

Non-rechargeable

21
Q

Separate Q. Name the component that contains chemicals that react to produce electricity.

A

A cell

22
Q

Separate Q. Why do non-rechargeable batteries stop working?

A

Chemical reactions inside the battery stop when one of the reactants has been used up.

23
Q

Separate Q. How are rechargeable batteries recharged?

A

A electrical current is supplied to the battery that reverses the chemical reaction inside.

24
Q

Separate Q. Describe how a fuel cell works

A
  • An external source of fuel (e.g. Hydrogen, Oxygen or Air) goes into the fuel cell.
  • The fuel is oxidised electrochemically
  • To produce a potential difference
25
Q

Separate Q. What reaction takes place inside a Hydrogen Fuel Cell?

A
  • Oxidation reaction.
  • Hydrogen is oxidised to produce water.
26
Q

Separate Higher Q. Write the half equations at the anode and cathode of a Hydrogen Fuel Cell.

A

• Anode (negative electrode *different to electrolysis):

H2 → 2H+ + 2e-

• Cathode (positive electrode *different to electrolysis):

O2 + 4H+ + 4e- → 2H2O

27
Q

Separate Q. List some advantages of Hydrogen Fuel cells as an alternative to rechargeable batteries and cells.

A
  • Fuel cells are less expensive than rechargeable batteries.
  • Rechargeable batteries need to be replaced after so many charges.
  • Fuel cells store more energy than rechargeable batteries.
28
Q

Separate Q. List some advantages of using Hydrogen Fuel Cells in cars as an alternative to conventional fuels.

A
  • Using fuel cells does not use up finite resources (e.g. fossil fuels).
  • Fuel cells don’t produce pollutants, they only produce clean water.