C3.2 Flashcards

1
Q

What is an exothermic reaction?

A

A reaction that transfers energy to the surroundings, increasing the temperature.

Examples: Combustion, oxidation, neutralization, hand warmers.

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2
Q

What is an endothermic reaction?

A

A reaction that takes in energy from the surroundings, decreasing the temperature.

Examples: Thermal decomposition, reaction of citric acid with sodium hydrogen carbonate, sports injury packs.

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2
Q

How can you identify an exothermic reaction on a reaction profile?

A

The products have lower energy than the reactants, and the energy change arrow points downwards.

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2
Q

How can you identify an endothermic reaction on a reaction profile?

A

The products have higher energy than the reactants, and the energy change arrow points upwards.

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2
Q

What is activation energy?

A

The minimum amount of energy that particles need to collide and react.

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2
Q

What happens to bonds during a chemical reaction?

A

Breaking bonds requires energy (endothermic).

Forming bonds releases energy (exothermic).

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2
Q

How do reaction profiles show activation energy?

A

It is the energy peak that reactants must reach before forming products.

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2
Q

How do you calculate the overall energy change of a reaction?

A

Overall energy change = Energy required to break bonds − Energy released when forming bonds.

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3
Q

What does it mean if the energy required to break bonds is greater than the energy released forming bonds?

A

The reaction is endothermic.

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3
Q

What does it mean if the energy released when forming bonds is greater than the energy required to break bonds?

A

The reaction is exothermic.

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3
Q

Why are hand warmers exothermic?

A

They release heat as the chemical reaction transfers energy to the surroundings.

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3
Q

Why are sports injury packs endothermic?

A

They absorb heat from the surroundings, cooling the affected area.

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4
Q

How do you recognize activation energy on a reaction profile graph?

A

It is the energy difference between the reactants and the peak of the curve.

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5
Q

What are the units of energy change in reactions?

A

Kilojoules per mole (kJ/mol).

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6
Q

Why do exothermic reactions feel hot?

A

Heat is transferred from the reaction to the surroundings, increasing temperature.

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7
Q

Why do endothermic reactions feel cold?

A

Heat is absorbed from the surroundings, reducing the surrounding temperature.

8
Q

How do you know if a reaction is reversible?

A

If it can go both ways, with products able to convert back to reactants under certain conditions. Represented by a double arrow (⇌).

9
Q

What is a reaction profile?

A

A diagram that shows the energy of reactants and products, the activation energy, and the overall energy change.

9
Q

Why is the activation energy important in a chemical reaction?

A

It determines the rate of reaction — higher activation energy means fewer particles have enough energy to react.

10
Q

What type of reaction is combustion?

A

Exothermic, as it releases heat when substances burn.

11
Q

What is thermal decomposition, and is it exothermic or endothermic?

A

Thermal decomposition is when a compound breaks down due to heat. It is an endothermic reaction because heat is absorbed.

11
Q

How does bond energy relate to reaction type?

A

If more energy is required to break bonds than to make bonds, the reaction is endothermic.

If more energy is released in making bonds, it is exothermic.

12
Q

Why are catalysts useful in reactions with high activation energy?

A

Catalysts lower the activation energy, allowing reactions to occur more easily and faster.

13
Q

What is the bond energy of a chemical bond?

A

The amount of energy needed to break 1 mole of a particular bond in kilojoules (kJ/mol).

14
Q

How do you experimentally determine if a reaction is exothermic or endothermic?

A

Measure the temperature change of the surroundings during the reaction.

Increase = Exothermic

Decrease = Endothermic