Fuels and Heats of reaction Flashcards
Hydrocarbon
A compound that contains only carbon and hydrogen
Saturated compound
a compound in which there are only single bonds between the atoms in the molecule
Unsaturated compound
One which contains at least one double or triple bonds netweem the atoms in the molecule
Structural isomers
Compounds with the same molecular formula but different structural formulae
Aliphatic (compound)
An organic compound that consists of straight (open) chains of carbon atoms and closed chain compounds with similar properties
Aromatic (compound)
An organic compound that contains a benzene ring structure in their molecules
Octane Number
Octane number of a fuel is a measure of the tendency of the fuel to resist knocking
Catalytic cracking
The breaking down of long chain hydro-carbon molecules into short chain molecules by heat and catalysts
Auto-ignition
Premature ignition (explosion) of the petrol-air mixture before normal ignition of the mixture by a spark takes place
Alkanes
These compounds are a family of hydrocarbons in which all atoms are linked by single bonds (saturated compounds)
Alkanes - formula
Cₙ H₂ₙ₊₂
Order
Meth Eth Prop But Pent Hex Hept Oct Non Dec
Alkane structual and condensed formulas
on hardback
Alkenes - formula
Cₙ H₂ₙ
Alkenes
- A homologous series of aliphatic hydrocarbons
- Lowest member of the series is ethene (2 carbon atoms)
- Each alkene molecule contains a carbon-carbon double bond
- Unsaturated compounds
Alkenes - methene
No methene due to double bonds
Alkynes endings
ends in -yne
Alkynes
Contain a carbon-carbon triple bond
Highly unsatured
Alkynes formula
Cₙ H₂ₙ₋₂
Ethyne
Name - Ethyne
Formula - C₂ H₂
Structural formula: H - C = C - H
Ethyne is the first of the series as you must have a carbon-carbon triple bond. (You need at least 2 carbons)
Endothermic reaction
Energy + reactants –> products
Activation energy
Activation energy is the maximum point on the reaction graph
Example of exothermic reaction and endothermic reaction
Exothermic reaction: Hydrochloric acid + magnesium
Endothermic reaction: water + ammonium nitrate
Bomb calorimeter
- use
- method
Used to find accurate values for heats of combustion
- Sample is ignited using electrically heated wire
- Excess oxygen ensures complete combustion of sample
- Heat produced by rapid + complete combustion of the sample heats, water + temperature is recorded
- Apparatus is well insulated to prevent heat loss
- Amount of heat used to start burning can be calculated and removed
Bond energy
- Average C-H bond energy in methane: 412 kJ mol⁻¹ ie. E(C-H) = 412 kJ mol⁻¹
- Energy of a particular bond can vary
- It is unusual to quote the average bond energies
Natural gas
- A colourless, odourless mixture of gases made up mostly of methane (CH₄). Other gases that can form part of natural gas include small amounts of ethane (C₂ H₆), propane (C₃ H₈), and butane (C₄ H₁₀)
- Methane burns relatively cleanly to produce heat energy + by-products of water and carbon dioxide
Why is natural gas useful?
- high kg calorific value
- Plentiful
- Easily distributed
Why mercaptans are added to natural gas
Due to natural gas being highly inflammable + explosive, mercaptans are added so it can be detected
Fractional distillation
A large-scale, continuous process which separates crude oil into a number of useful mixtures called fractions
eg. refinery gas is a fraction that can be used as a domestic gas
Octane number
Measure of the tendency of the fuel to resist knocking
eg. 2, 2, 4 - trimethlypentane is assigned an octane number of 100
heptane is assigned an octane number of 0
Factors affecting octane numbers
The shorter the alkane chain, the more branched the chain, and cyclic compounds all lead to higher octane numbers
Methods used to increase the octane number of petrol
- Isomerisation
- Catalytic cracking
- Dehydrocyclisation
- Adding oxygenates
Ways of manufacturing hydrogen
- steam reforming of natural gas
- electrolysis of water
Isomerisation
involves changing straight-chained hydrocarbons into branched-chained isomers. The branched-chained isomers burn more smoothly, therefore have higher octane number.
Catalytic cracking
involves breaking down long chained hydrocarbons (low demand) into short chained molecules (high demand). Short-chained hydrocarbonsa higher octane number + tend to be highly branched.
Dehydrocyclisation
involves conversion of straight chained hydrocarbons to form ring compounds. Then converted into aromatic compounds. Done in presence of a catalyst. As hydrogen is a byproduct of this reaction it is called ‘dehydro’. Aromatic compounds have high octane number but also carcinogenic.
Adding oxygenates
the addition of oxygen compounds to the petrol.
Tend to be of two types (a) addition of alcohols i.e. methanol (octane no. of 114) and (b) addition of ethers i.e. methyl tert-butyl ether (MTBE) (octane no. of 118).
These compounds (a) increase octane number of the petrol (b) cause less pollution as they reduce level of carbon monoxide in exhaust fumes.
Catalytic cracking allows what?
Allows large hydrocarbon molecules to be broken down into smaller, more useful hydrocarbon molecules
Catalytic cracking method
Fractions containing large hydrocarbon molecules are vaporised + passed over a hot catalyst. This breaks chemical bonds in the molecules + forms smaller hydrocarbon molecules
Why do catalytic cracking
Fuels made from oil mixtures w/ large hydrocarbon molecules -> not efficient, do not flow easily, difficult to ignite
Crude oil –> often too many large hydrocarbon molecules + not enoughh small hydrocarbon molecules to meet demand
Heat of neutralisation
- Nearly always exothermic (-△H)
- Measured in kJ/mol or kJ mol⁻¹
- Always less than -57 kJ mol⁻¹
WRITE A NEGATIVE IN FRONT OF THE ANSWER IF ASKED TO CALCULATE HEAT OF NEUTRALISATION
How to find out if substance is acid or base
Acid: contains H⁺ ions eg. HCl
Base: Contains OH eg. NaOH
Calculating the heat liberated in a reaction
Heat liberated/given out = mass x specific heat capacity x rise in temperature
(m x c x (t₂ - t₁)
mass - kg
shc - J kg⁻¹ K⁻¹
Mercaptans
Chemicals added to odourless gases to give them an unpleasant smell so that gas leaks can be detected
Who discovered benzene?
Michael Faraday in 1825
Properties of benzene
Formula: C₆ H₆
Highly unsaturated
Highly toxic
Carcinogenic
Points about benzene that puzzled chemists
- Reactivity
2. Bond lengths
- Reactivity of Benzene
Predicted benzene could be highly reactive. Found to be very unreactive.