Enthalpy Flashcards

1
Q

What is enthalpy?

A

The measure of heat energy within a chemical system

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2
Q

How do you calculate enthalpy change?

A

Enthalpy of products - Enthalpy of reactants

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3
Q

Where is energy transferred in an exothermic change?

A

Energy is transferred from system to the surroundings

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4
Q

Where is energy transferred in an endothermic change?

A

Energy is transferred from the surroundings to the system

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5
Q

What are 4 key features of an exothermic reaction?

A

Enthalpy change is negative
Chemical system loses energy
Surroundings gain energy
Temperature of surroundings increases

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6
Q

What are 4 key features of an endothermic reaction?

A

Enthalpy change is positive
Chemical system gains energy
Surroundings lose energy
Temperature of surroundings decreases

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7
Q

What is activation energy?

A

The minimum energy required for a reaction to take place

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8
Q

What are standard conditions?

A

25 C or 298K
100kPa
1 mol dm^3

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9
Q

Define standard enthalpy change of formation

A

Enthalpy change when one mole of a substance is formed from its constituent elements with all substances in their standard states

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10
Q

What is the enthalpy change of formation for all elements?

A

0

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11
Q

Define standard enthalpy change of combustion

A

Enthalpy change when one mole of a substance undergoes complete combustion in oxygen with all substances in standard states

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12
Q

Define standard enthalpy change of neutralisation

A

Enthalpy change when 1 mole of water is formed in a reaction between an acid and alkali under standard conditions

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13
Q

What is 0 degrees C in K?

A

273K

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14
Q

Define specific heat capacity

A

The energy required to raise the temperature of 1g of a substance by 1K

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15
Q

What is the specific heat capacity of water?

A

4.18

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16
Q

What is the equation for calculating heat energy?

A

Q= mc delta T

17
Q

Give reasons for inaccuracy in heat energy of combustion practical

A

Heat energy lost to the surroundings
Incomplete combustion
Evaporation of alcohol from the wick
Non standard conditions

18
Q

How would you minimise effect of heat loss or incomplete combustion?

A

Draught screens

Input of oxygen gas

19
Q

What piece of equipment is used to measure enthalpy change of reaction between two solutions?

A

Polystyrene cups

20
Q

Define ‘Average Bond Enthalpy’

A

Energy required to break one mole of a specified type of bond

21
Q

Are bond enthalpies exothermic or endothermic?

A

Endothermic (always have a positive value)

22
Q

What is an average bond enthalpy calculated from?

A

Actual bond enthalpies in different environments

23
Q

Bond breaking- exothermic or endothermic?

A

Endothermic

24
Q

Bond making- exothermic or endothermic?

A

Exothermic

25
What determines whether a reaction is overall exothermic or endothermic?
The difference between the value for making the bond and value for breaking bonds
26
How is enthalpy change calculated from bond enthalpies?
Bond enthalpies in reactants - Bond enthalpies in products
27
What are the limitations for using average bond enthalpies?
The bond enthalpies are slightly different in each environment, however not a major difference as an average bond enthalpy is used. Need all molecules to be gaseous
28
What does 'Hess' Law' state?
If a reaction can take place by two routes, and starting and finishing conditions are the same, the total enthalpy change is the same for each route