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Summary A Level Chemistry Edexcel Unit 8 - Energetics I notes written by a 3A* Imperial College London Medicine Student CA$5.48   Add to cart
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Summary A Level Chemistry Edexcel Unit 8 - Energetics I notes written by a 3A* Imperial College London Medicine Student

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  • Course
  • Unit 8 - Energetics I
  • Institution
  • PEARSON (PEARSON)
  • Book
  • George Facer\'s Edexcel A Level Chemistry Student Book 1

Detailed notes on Unit 8 - Energetics I covering all the specification points, and allowed me to achieve an A* in chemistry. Covers enthalpy changes, thermochemical equations, Hess's law, Hess cycles, example calculations, standard enthalpy of formation, reaction, combustion, neutralisation and ato...

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Document information

  • No
  • Chapter 13 energetics (topic 8)
  • March 26, 2023
  • 17
  • 2022/2023
  • Summary

Subjects

  • thermodynamics
  • energy
  • joule
  • specific heat capacity
  • enthalpy
  • enthalpy changes
  • exothermic
  • endothermic
  • standard enthalpies
  • formation
  • reaction
  • combustion
  • neutralisation
  • bond enthalpy
  • atomisa
  • hesss law

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  • PEARSON (PEARSON)
  • Chemistry 2015
  • Unit 8 - Energetics I
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8-Energetics 1
Enthalpy Change
Thermochemical Equations
Hess’s Law
Standard Enthalpies
Standard Enthalpy of Reaction (ΔHr ⦵)
Practical: Calculation of Enthalpy of Reaction from an Experiment using an Insulated
Container
Standard Enthalpy of Combustion (ΔHc ⦵)
Practical: Experimental Method to Find the Enthalpy of Combustion of a Liquid
Calculation of Standard Enthalpy of Formation from Combustion
Standard Enthalpy of Neutralisation (ΔHne u t ⦵)
Practical: Experimental Method to find the Enthalpy of Neutralisation of an Acid
Standard Enthalpy of Atomisation (ΔHa ⦵)
Bond Enthalpy (ΔHB )
Calculation of Enthalpy of Reaction from Average Bond Enthalpies
Enthalpy Titrations



Law of Conservation of Energy - Energy can neither be
created nor destroyed, converted from one form to another.

Unit of energy - joule (J) or kilojoule (kJ).




8-Energetics 1 1

, Heat Transferred = Mass x Specific Heat Capacity x Temperature
Change

Q=mcΔT

Specific heat capacity of water - 4.18Jg− 1o C− 1 .

Specific Heat Capacity:

The energy required to increase the temperature of one gram of a substance by
one degree kelvin. Units - J K− 1 g− 1 .

Example:

Calculate the heat required to increase the temperature of 100cm3 of water from
17.6o C to 50.5o C.

ΔT = 50.5-17.6 = 32.9o C

Q=mcΔT

Q = 100 x 4.18 x 32.9

Q = 13,800J / 13.8kJ



Enthalpy Change
Enthalpy (H) of a system:
The enthalpy change (Δr H) for a reaction is the heat energy change measured
out under conditions of constant pressure.

The release or absorption of heat energy by a system at constant pressure
is caused by a change in the enthalpy of the chemicals.

Absolute enthalpy values cannot be found.

ΔH = (enthalpy of products) - (enthalpy of reactants).

ΔH = Hp - Hr

Heat Energy Change in a reaction (Q):

Can be measured experimentally using Q=mcΔT, where m is the mass of the
substance that has a temperature change ΔT and a specific heat capacity c.

Calorimetry:




8-Energetics 1 2

, The measurement of the heat required or absorbed by chemical reactions.

Exothermic Reactions:

Reactants have a higher enthalpy than the products.

The system loses energy during the reaction.

The value of ΔH is negative.

Energy is transferred to the surroundings as heat - surrounding increase in
temperature.




Endothermic Reactions:

Reactants have a lower enthalpy than the products.

The system gains energy during the reaction.

The value of ΔH is positive.

Energy is transferred from the surroundings as heat - surroundings decrease
in temperature.




Thermochemical Equations
Thermochemistry:




8-Energetics 1 3

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