5) Chemical energetics Flashcards

1
Q

Enthalpy

A
  • the total chemical energy inside a substance
  • can be endothermic (+) or exothermic (-)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Differences between endothermic and exothermic reactions

A

table in notes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Transition state

A

stage during reaction at which chemical bonds are partially broken and formed (very unstable and is higher in energy than the reactants and products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Activation energy (Ea)

A

minimum amount of energy needed for reactant molecules to have a successful collision and start the reaction (energy needed to reach the transition state)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Standard conditions

A

Pressure- 101kPa
Temp- 298K (25 degrees Celsius)
Each substance involved in the reaction is in its normal physical state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Standard enthalpy change of reaction

A
  • The enthalpy change when the reactants in the stoichiometric equation react to give the products in their standard states
  • Exothermic and endothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Standard enthalpy change of formation (commonly asked)

A
  • The enthalpy change when 1 mole of a compound is formed from its elements in their standard states
  • Exothermic and endothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Standard enthalpy change of combustion

A
  • The enthalpy change when 1 mole of a substance is burnt in excess oxygen in their standard states
  • Exothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Standard enthalpy change of neutralisation

A
  • The enthalpy change when 1 mole of water is formed by reacting an acid and alkali in their standard states
  • Exothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Bond energies

A
  • enthalpy changes take place, because bonds are being broken and formed
  • energy in the form of heat is needed to overcome attractive forces between atoms, therefore bond breaking is endothermic
  • energy released from the reaction to surroundings in the form of heat when new bonds are formed, therefore bond formation is exothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Enthalpy change of reaction formula

A

enthalpy change for bonds broken + enthalpy change for bonds formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Enthalpy change of formation formula

A

energy of products - energy of reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Exothermic rxn

A
  • if more energy is released when new bonds are formed than energy is required to break bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Endothermic rxn

A
  • if more energy is required to break bonds than energy is released when new bonds are formed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Measuring enthalpy changes

A
  • a calorimetry is a technique used to measure changes in enthalpy of chemical reactions
  • a calorimeter can be made up of a polystyrene drinking cup, a vacuum flask or a metal can
  • the energy transferred as heat can be calculated by q= m x c x triangle T
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Specific heat capacity

A

the energy required to increase the temperature of 1g of a substance by 1 degree Celcius

17
Q

Formula to calculate any changes in enthalpy per mole of a reactant or product

A

enthalpy change= m x c x triangle T
- when there is a rise in temp, the value for enthalpy change becomes - suggesting the reaction is exothermic
- then there is a fall in temp, the value for enthalpy change becomes + suggesting the reaction is endothermic

18
Q

Hess’s law

A

the total enthalpy change in a chemical reaction is dependent on the route by which the chemical reaction takes place as long as the initial and final conditions are the same

19
Q

Example of hess’s cycle for enthalpy change of formation

A

in notes

20
Q

Example of hess’s cycle for enthalpy change of combustion

A

in notes

21
Q

Hess’s cycle- mean bond enthalpy

A

in notes

22
Q

Calorimetry (combustion energy transferred)

A

1) Calculate energy first (substitute all the values into equation)
2) Calculate n of fuel to work out enthalpy (mass/Mr)
3) Enthalpy= first answer/n

  • if there is a rise in temp it will be negative (exothermic)
    *if there is a fall in temp it will be positive (endothermic)
23
Q

Calorimetry (of solutions)

A
  • polystyrene cup is used to prevent heat loss
  • add acid first- measure temp
  • add alkali/solid- stir and measure temp change
  • similar formula to work out enthalpy change