Enthalpy Changes Flashcards

1
Q

What does system mean in a chemical reaction?

A

The atoms and bonds involved in the chemical reaction.

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2
Q

Explain the law of conservation.

A

The amount of energy in an isolated system remains the same. Energy cannot be created or destroyed, it can only be transferred from one form to another.

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3
Q

What energy change is breaking bonds associated with?

A

Energy is taken in to break bonds —> endothermic reaction

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4
Q

What energy change is making bonds associated with?

A

Energy is released to make bonds —> exothermic reaction

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5
Q

What is an endothermic reaction?

A

A reaction with an overall positive enthalpy change (+ΔH) —> enthalpy of products > enthalpy of reactants

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6
Q

What is an exothermic reaction?

A

A reaction with an overall negative enthalpy change (-ΔH) —> enthalpy of products < enthalpy of reactants

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7
Q

What does activation energy mean?

A

The minimum energy required for a reaction to take place

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8
Q

What are the standard conditions?

A

100 kPa
298 K

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9
Q

What does ‘in standard state’ mean?

A

The state and element / compound exists at in standard conditions

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10
Q

Define enthalpy change of formation.

A

The energy change that takes 1 mole of a compound is formed from its constituent elements in their standard state under standard conditions

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11
Q

Define enthalpy change of combustion

A

The energy change that takes place when 1 mole of a substance is completely combusted.

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12
Q

Define enthalpy change of neutralisation

A

The energy change that takes place when 1 mole of water is formed from a neutralisation reaction.

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13
Q

What does the enthalpy change of reaction mean?

A

The energy change associated with a given reaction.

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14
Q

What are the advantages of using a bomb calorimeter? (2)

A
  • minimises heat loss
  • pure oxygen used —> ensures complete combustion
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15
Q

Why might experimental methods for enthalpy determination not be accurate?

A

Heat is lost to surroundings
Not in standard conditions
Reaction mau not go to completion

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16
Q

What does average bond enthalpy mean?

A

The mean energy required to break 1 mole of bonds in gaseous molecules.

17
Q

Why will using bond enthalpies not be as accurate as using standard enthalpy of combustion/formation?

A

Bond enthalpies are a mean for the same bond across different molecules whereas standard enthalpy of combustion and formation apply just to that molecule, therefore they are more accurate.

18
Q

How to calculate enthalpy change of reaction using average bond enthalpies?

A

ΔH = Σ(bond enthalpies of reaction) — Σ(bond enthalpies of products)