steeper line \= faster rate flat \= reaction finished higher line \= more reactants and products
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collision theory in rate of reaction
1. collision frequency of reacting particles more collisions \= faster rate
2. energy transferred during a collision particles need to collide with enough energy to be successful
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factors affecting rate of reaction
1. temperature particles have more energy, collide more frequently
2. concentration or pressure more particles in an area \= more frequent collisions
3. surface area smaller pieces \= more area for collisions to happen on
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catalyst
a substance that speeds up the rate of reaction without being used up itself
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catalyst's affect on rate of reaction
speed it up by decreasing activation energy
do this by creating an alternative reaction pathway with lower activation energy
e.g. enzyme
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rate of reaction equation
amount of reactant used up or amount of product formed / time
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precipitate
a solid formed in a reaction
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precipitate and colour change showing rate of reaction
can observe how long it takes for a solution to lose or gain colour can observe how long it takes a solution to become cloudy
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change in mass showing rate of reaction
1. put reaction on scale 2. is a gas is produced, the mass will decrease 3. the quicker it decreases, the faster the reaction
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volume of gas showing rate of reaction
gas syringe to measure vol of gas being produced more gas given off in one time interval \= faster rate
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finding reaction rates from graphs
1. calculating mean rate overall change in y axis / total time taken
2. calculating rate at a point draw a tangent at the point and find the gradient
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reversible reaction
a + b ↔ c + d
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rate of reversible reactions
as reactants react, their concentration falls. (forward reaction slows) as products are made, their concentration rises (backward reaction speeds up)
eventually forward reaction is at same rate as backward reaction (equilibrium)
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equilibrium
both reactions are happening but there is no overall effect unchanging balance of products and reactants only occurs in a closed system
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position of equilibrium
equilibrium doesn't mean amounts of reactants are equal lies to left \= higher conc. of reactants lies to right \= higher conc. of products
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conditions affecting position of equilibrium
temperature pressure (only in gases) concentration of reactants and products
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exothermic and endothermic reversible reactions
if endothermic in one direction, exothermic in other energy transferred from surroundings \= energy transferred to surroundings
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Le Chatelier's Principle
if you change the conditions of a reversible reaction at equilibrium, the system will try to counteract that change
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changes to temperature
decrease temp \= equilibrium will more to exothermic direction to create more heat vice versa for increase temp
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changes to pressure
only for gases increase pressure \= equilibrium moves to side with lower molecules of gas vice versa for decrease pressure
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changes to concentration
change concentration \= no more equilibrium increase conc. of reactants \= makes more products decrease conc. of products \= less reactants etc
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hydrocarbon
any compound formed from carbon and hydrogen only
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alkane formula
Cn H2n+2
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alkanes are saturated
each carbon bonds to four other atoms
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homologous series
a series of compounds that have similar properties and the same general formula
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saturated
bonded with the maximum amount of atoms
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first alkane
methane CH4
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second alkane
ethane C2H6
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third alkane
propane C3H8
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fourth alkane
butane C4H10
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the shorter the hydrocarbon chain...
the less viscous the more volatile the more flammable lower boiling points
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complete combustion
happens in excess of oxygen releases lots of energy C and H from the hydrocarbon are oxidised
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complete combustion equation
hydrocarbon + oxygen \= carbon dioxide + water
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crude oil
fossil fuel formed from remains of plats and animals remains turn to oil with time, temp, and pressure non-renewable finite mixture of lots of different hydrocarbons
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fractional distillation
used to separate hydrocarbon fractions
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uses of crude oil
fuel - kerosene, diesel etc makes new compounds like polymers and solvents
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cracking
splitting up hydrocarbons turns long chain hydrocarbons into shorter chains
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catalytic cracking
1. vaporise hydrocarbon 2. pass over hot powered aluminium oxide catalyst
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steam cracking
1. vaporise hydrocarbon 2. mix with steam 3. heat to a very high temperature
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thermal decomposition
breaking down molecules by heating them
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cracking products
shorter chain hydrocarbon + alkene
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alkene
hydrocarbons with a double bond between two carbons in their chain two fewer hydrogens than alkanes
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properties of alkenes
unsaturated c\=c bond can open to bond to other atoms much more reactive than alkanes
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alkene formula
Cn H2n
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first alkene
ethene C2H4
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second alkene
propene C3H6
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third alkene
butene C4H8
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fourth alkene
pentene C5H10
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incomplete combustion
combustion when there isn't enough oxygen in the air smoky yellow flame less energy released happens in alkenes
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incomplete combustion equation
alkene + oxygen \= carbon + carbon monoxide + water
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functional group
group of atoms in a molecule that determine how that molecule typically reacts
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alkane functional group
c-c
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alkene functional group
c\=c
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alcohol functional group
-OH
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carboxylic acid functional group
-COOH
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ester functional group
-COO-
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alkene addition reaction
the c\=c double bond opens up, allowing a new atom to be added to each carbon
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alkene + hydrogen
hydrogenation hydrogen reacts with c\=c to form equivalent alkene needs a catalyst e.g. ethene + H2 \= ethane
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alkene + steam
alcohol is formed water added across double bond needs a catalyst e.g. ethene + steam \= ethanol
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halogens + alkenes
addition reaction with halogen each c\=c atom bonds with a halogen atom e.g. bromine + ethene \= dibromethane
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polymers
long chains of monomers (plastics) normally carbon based monomers normally alkenes
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polymerisation
monomers becoming polymers needs high pressure and a catalyst
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addition polymers
made from unsaturated monomers c\=c bond opens up to join to another opened up carbon atom makes polymer chains poly(name of monomer)
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addition polymer diagram
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alcohol general formula
Cn H2n+1 OH
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first alcohol
methanol CH3OH
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second alcohol
ethanol C2H5OH
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third alcohol
propanol C3H7OH
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fourth alcohol
butanol C4H9OH
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alcohol properties
flammable undergo complete combustion in air first 4 alcohols soluble in water to make pH 7 react with sodium. 1 product is hydrogen oxidised to produce carboxylic acids
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alcohol uses
solvents because they dissolve things water can't fuels e.g. spirit burners because they burn cleanly
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fermentation
using an enzyme in yeast to convert sugars into ethanol
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fermentation equation
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fermentation conditions
fastest at 37ºc and in slightly acidic conditions no oxygen
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first carboxylic acid
methanoic acid HCOOH
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second carboxylic acid
ethanoic acid CH3COOH
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third carboxylic acid
propanoic acid C2H5COOH
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fourth carboxylic acid
butanoic acid C3H7COOH
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carboxylic acids + carbonates
\= salt + water + carbon dioxide
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carboxylic acids properties
dissolve in water dont ionise completely weak acids (higher pH)
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ester equation
alcohol and carboxylic acid acid catalyst (e.g. sulfuric acid)
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first ester
ethyl ethanoate CH3COOC2H5
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condensation polymers
polymers containing different functional groups monomers form bonds e.g. polyester
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molecule lost during condensation polymerisation
e.g. water
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condensation polymer example
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number of types of monomers
addition - one monomer type condensation - two monomer types with diff func groups or one monomer with 2 functional groups
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number of products
addition - 1 product condensation - 2 products
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functional groups involved in polymerisation
addition - c\=c double bond condensation - two reactive groups per monomer
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amino acids
amino group + carboxyl group
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amino acids form...
polymers called polypeptides via condensation polymerisation
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long chains of polypeptides
proteins
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natural occurring polymers
DNA proteins carbohydrate polymers (e.g. cellulose and starch)