Topic 14 - Energetics Flashcards Preview

Grace Chemistry IGCSE > Topic 14 - Energetics > Flashcards

Flashcards in Topic 14 - Energetics Deck (14)
Loading flashcards...
1
Q

What is enthalpy change represented as

A

ΔH

2
Q

What are the units for enthalpy change

A

kJ/mol

3
Q

define endothermic

A

Reactions that take in energy from their surroundings (+ΔH)

4
Q

Define exothermic

A

Reactions that transfer heat energy to the surroundings (-ΔH)

5
Q

How do you calculate ΔH from bond energies

A

Bonds broken - bonds made

Breaking bonds is an endothermic reaction because energy must be supplied

Making bonds is an exothermic reaction because energy is released

6
Q

describe the method for calorimetry; combustion

A

1) put 50g water in a copper can
2) measure the initial temperature of the water, and the initial mass of the spirit burner and lid
3) put the spirit burner underneath the can and light the wick, burn for 30s while stirring constantly
4) put out the taken using the burner lid, measure the final temperature of the water and the final mass of the burner and lid
5) reduce heat loss to atmosphere by using a screen to act as a draught excluder, don’t do it next to an open window

7
Q

What is change in energy represented as

A

ΔE

8
Q

How do you calculate change in energy (J)

A

ΔE = mass of water x SHC x ΔT of the water

9
Q

How do you calculate enthalpy change

A

-ΔE
ΔH = ———
moles

10
Q

Why is calorimetry so inaccurate

A
  • heat loss to atmosphere

* incomplete reaction

11
Q

What is enthalpy change?

A

The overall change in energy in a reaction

Measured in kJ/mol

Exothermic reactions give negative enthalpy change

Endothermic reactions give positive enthalpy change

12
Q

What is a reaction profile?

A

Diagrams which show the relative energies of the reactants and products in a reaction, and how the energy changes over the course of the reaction

The difference in height between the reactants and the products show the energy given out/taken in

The initial rise in energy represents the activation energy (the minimum amount of energy the reactants need to collide with each other and react)

In exothermic reaction profiles, the products are at a lower energy than the reactants

In endothermic reactions the products are at a higher energy than the reactants

13
Q

Describe the general method for calorimetry: dissolving, displacement and neutralisation reactions

A

*general theory- take the temperature of reactants (making sure they’re the same), mix them and measure the temperature of the products)

1) mix the reactants in a polystyrene cup
2) reduce energy loss to the surroundings by putting the polystyrene cup into a beaker of cotton wool to give it more insulation, and putting a lid on the cup to reduce energy lost by evaporation

14
Q

Describe the calorimetry neutralisation reaction

A

1) put 25cm3 of hydrochloride acid and sodium hydroxide into separate beakers
2) place the beakers in a waterbath at 25°C until they both reach this temperature
3) add the HCl followed by the NaOH to a polystyrene cup with a lid
4) take the temperature of the mixture every 30s, record the highest temperature