Unit 3 - Lesson 13: Endothermic and Exothermic Reactions Flashcards

1
Q

Define an exothermic reaction.

A

An exothermic reaction is one which gives out energy to the surroundings, usually in the form of heat and usually shown by a rise in temperature of the surroundings.

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2
Q

Define an endothermic reaction.

A

An endothermic reaction is one which takes in energy to the surroundings, usually in the form of heat and usually shown by a fall in temperature of the surroundings.

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3
Q

What happens to particles when applying thermal energy (heat) to them?

A

Thermal energy causes particles to move (gain kinetic energy). The more thermal energy, the more kinetic energy. The more particles move, the more intermolecular forces and/or bonds can break.

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4
Q

What is a reaction if it needs heat or speeds up when heat is applied?

A

Endothermic.

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5
Q

Give an example of endothermic reactions.

A

Sublimation. Apply heat to a solid and the particles will move so much, the intermolecular bonds break, forming a gas.

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6
Q

Is thermal decomposition of a metal carbonate endothermic or exothermic?

A

Endothermic. Heat breaks down the substance.

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7
Q

What kind of reaction is it if there is a temperature decrease?

A

Endothermic reaction.

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8
Q

What do we use endothermic reactions in? (Think daily life)

A

Handwarmers, cold packs & self-heating food/mugs.

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9
Q

Are combustion reactions exothermic or endothermic?

A

Exothermic. They produce thermal energy. For example:
2Mg + O2 –> 2MgO
S + O2 –> SO4
H + O2 –> H2O

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10
Q

Give three examples of reactions that are exothermic.

A
  1. Reactions between metals and acid
  2. Neutralisation reactions
  3. Displacement reactions
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11
Q

What are displacement reactions?

A

Displacement reactions are two elements ‘fighting’ for something (displace it from a compound). The most reactive will win.

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12
Q

What does the thermite reaction involve?

A

Two metals ‘fighting’ for an oxide. For example:
Aluminium + Iron (III) Oxide –> Iron + Aluminium Oxide
2Al + Fe2O3 –> 2Fe + Al2O3
Aluminium is higher up the reactivity series than iron, so it steals the oxide (displaces the iron). Pure iron is produced. Iron can be extracted with carbon. This is a redox reaction. Iron is reduced. Aluminium is oxidised.

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13
Q

What kind of reaction (endothermic/exothermic) is it if there is a temperature increase?

A

Exothermic reaction.

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14
Q

What is ‘Enthalpy’?

A

Enthalpy is the total heat energy in a reaction. This is the overall change in energy during the reaction.

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15
Q

What is enthalpy measured in?

A

Joules (J)

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16
Q

What letter stands for enthalpy?

17
Q

What does the Greek letter ‘delta’ (Δ) stand for?

A

‘Change in’

18
Q

How can enthalpy change be calculated?

A

Energy in product - Energy in reactant = Enthalpy change

19
Q

Do exothermic reactions lose or gain energy?
b) What does this say about their ΔH?

A

Lose.
b) Therefore, their ΔH is always negative.

20
Q

Do endothermic reactions lose or gain energy?
b) What does this say about their ΔH?

A

Gain.
b) Therefore, their ΔH is always positive.

21
Q

What is enthalpy change (ΔH) measured in?

A

kJ/mol (kilojoules per mole). This is the amount of kJ lost or gained for every 1 mole of reactant. Occasionally, it’s written as kJ mol^-1.

22
Q

Why are endothermic ΔH positive?

A

Because they take in energy.

23
Q

Why are exothermic ΔH negative?

A

Because they release energy.