CHEMISTRY PART 1 and 2 Flashcards
What is the mass number (top)?
Total number of protons and neutrons
What is the atomic number (bottom)?
Total number of protons
How do you work out the number of neutrons?
Mass number (top) subtract the atomic number (bottom)
How do you work out the number of electrons?
They are equal to the number of protons (atomic number)
What is the mass of a proton?
1
What is the mass of an electron?
Very small
What is the mass of a neutron?
1
What is the charge of an electron?
Negative (-1)
What is the charge of a proton?
Positive (+1)
What is the charge of a neutron?
Neutral (0)
What are compounds?
When atoms of two or more elements are chemically combined together
What is an isotope?
Different atomic forms of the same element which have the SAME number of PROTONS but a DIFFERENT number of NEUTRONS
Isotopes have different … numbers
Mass (top)
When are ions formed?
When there is a full outer shell of electrons
Ionic compounds always have …
Giant ionic lattices
How are the ions arranged in a regular lattice?
The ions are closely packed
Ionic bonding is the … of electrons
Transferring
Ionic bonding takes place between which materials?
Metals and non metals
Why are there strong electrostatic forces of attraction between ions?
The opposite charges between the ions attract to each other
Why are salt crystals in a cuboid shape?
The single crystal of sodium chloride is one giant ionic lattice
Why do ionic compounds have a high MP and BP?
It takes a large amount of energy to overcome the electrostatic forces of attraction
When can an ionic substance conduct electricity?
When they melt, and their ions are free to move and carry the charge
Elements most likely to form ions are in groups
1
2
6
7
Ions have the electronic structure of a…
Noble gas
What happens in the ionic bonding of sodium chloride?
The single electron on Sodium’s outer shell transfers to become the 8th electron of Chlorine’s outer shell. Sodium becomes positively charged, Chlorine becomes negatively charged.
Na+
Cl-
Final product - NaCl
What happens in the ionic bonding of magnesium oxide?
The two electrons from Magnesium outer shell transfer to Oxygen’s outer shell that would’ve had 6 electrons. Magnesium becomes positively charged, oxygen becomes negatively charged.
Mg2+
02-
Final product - MgO
What happens in the ionic bonding of calcium chloride?
Calcium has two elections on its outer shell. Each goes to a chlorine atom which gain a single electron to complete the full outer shell. The chlorine's become negatively charged, and the calcium becomes positively charged. Ca2+ Cl- Cl- Final product - CaCl2
What is covalent bonding?
The sharing of electrons within a compound to achieve a full outer shell
Covalent bonding occurs with …
2 non metals
Covalent bonds have a … MP and BP
Low
Why do covalent bonds have low MP and BP?
The covalent bonds are strong but the intermolecular forces between the molecules are weak
How can you overcome the weak intermolecular forces in covalent bonds?
Boiling or melting the substances
Why can covalent bonds not conduct electricity?
They have no overall charge
There are no charge carriers (free electrons/free ions)
Examples of simple covalent bonded molecules (4)
Hydrogen
Oxygen
Methane
Chlorine
Boiling and melting points can depend on the…
Size and the shape of a molecule
Why does CH4 have a lower BP than CO2?
As the molecules cannot get as near to one another
What happens in the covalent bonding of Hydrogen?
Hydrogen have one electron and only require one more for a full outer shell.
Therefore they overlap to share two electrons between both.
What happens in the covalent bonding of chlorine?
Chlorine atoms have 7 electrons on their outer shell.
Therefore for the bonding of two chlorine atoms, they share their seventh electron where they overlap.
What happens in the covalent bonding of methane?
Carbon has four electrons on its outer shell.
Therefore it forms four covalent bonds with four hydrogen atoms.
Within the overlap there is one electron from hydrogen and one from chlorine (2 in total)
So chlorine has 8 electrons in total and all the hydrogens have a full outer shell too.
What happens in the covalent bonding of hydrogen chloride?
Hydrogen and chlorine both require only one more electron for a full outer shell.
Therefore, they share two electrons within the one overlap.
What happens in the covalent bonding of ammonia?
Nitrogen has 5 electrons on its outer shell. The final 3 of the 5 each form a covalent bond with a hydrogen atom.
Therefore, they all have a full outer shell.
What happens in the covalent bonding of water?
Oxygen has 6 electrons on its outer shell. It bonds with 2 hydrogen atoms.
Therefore there are two electrons in the overlap.
What happens in the covalent bonding of oxygen?
Both oxygen atoms have 6 electrons on its outer shell.
Two electrons from each are shared in the overlap (4 in total) to create a full outer shell.
Therefore, a double covalent bond is formed.
Most molecular substances are … at room temperature
Gases and liquids… although they CAN be solids
What are macromolecules?
Giant covalent structures or lagged covalent bonded molecules
General features of macromolecules
No charged ions
Do not conduct electricity even when molten (except graphite)
High MP and BP
Bonded by strong covalent bonds
Examples of macromolecules (3)
Diamond
Graphite
Silicon dioxide (silica)
Explain the features of diamond
Made up carbon Each carbon atoms forms four covalent bonds with other carbon atoms Rigid structure Hardest natural substance Used for drill tips
Explain the features of graphite
Each carbon atoms forms 3 covalent bonds - creating layers
The bonds are strong but intermolecular forces between the layers are weak
Layers slide which is how a pencil works
Soft and slippery
Only non metal that conducts heat electricity as each carbon atom has one free/delocalised electron
Properties of metals (7)
Conduct heat Conduct electricity Sonorous Ductile High MP and BP Hard Malleable
Define sonorous
Makes a ringing sound when hit
Define malleable
Can be hammered/ bent into different shapes
Define ductile
Can be drawn into wires
Metal properties are due to …
Free electrons
Where do free electrons in metals come from?
The outer shell of every atom in the giant structure
How do free electrons help the structure of a metal?
They hold the atoms together as the strong electrostatic forces attract the positive metal ions and negative metal ions
Why do metals have a high MP and BP?
The free electrons are negatively charged and therefore attract the positive ions by electrostatic forces.
The strong forces are difficult to overcome, hence the high BP and MP
Why can metals conduct electricity and heat?
The free ions are free to move and carry the charge
Why are metals malleable?
The position of ions can change because of the movement of free electrons
The layers of atoms can slide over each other allowing it to be bent/shaped
What are alloys?
A mixture of 2 or more metals, usually to create a material with more desirable properties
Why are alloys harder than pure metals?
Different sized elements have different sized atoms
Therefore a mixture of the two, distorts the the regular arrangement
This makes it difficult for the atoms to slide over each other
Therefor they are harder than pure metals
Examples of alloys (3)
Amalgam, mostly mercury, used in dental fillings
Brass, mostly copper and zinc, used in hinges/electrical plugs
Solder, mostly lead and tin, used to join metals
Smart alloys
Behave different/have unusual properties depending on conditions e.g. Temperature
Example of a smart alloy
Nitinol (nickel and titanium)
Metal alloy
If bent out of shape, it returns when heated or an electric current is passed through it
Useful for glasses frames and some dental braces
Fullerenes examples
Buckminister fullerene
Nanotube
Properties/ uses of buckminister fullerene
Hexagon shape, connected to make a sphere
Uses included drug delivery in body, lubricants and catalysts
Properties/ uses of nanotube
Light
Potentially strong
Tube structure of carbon in hexagons
Uses include reinforcing materials e.g tennis racket
Features of nanoparticles
VERY small 1-100nm across Include fullerenes Contain a few hundred atoms Different properties Very large surface area to volume ratio
Why do fullerenes make a good conductor?
They have a large surface area to volume ratio (for the amount of material, the surface area is huge)
Uses of nanoparticles
New industrial catalysts Highly specific sensors Stronger, lighter building materials Sun tan/deodorant Nanomedicine e.g. Drug delivery Lubricant coatings Electric circuits for computer chips
What determines the properties of plastics?
The forces between the molecules
What causes the atoms to be held together in long chains (in plastics)?
The strong covalent bonds
How do weak forces affect the chains in polymers?
They are held together by weak intermolecular forces and therefore become more tangled
They are free to slide over each other
How strong forces affect the chains in polymers?
They have stronger intermolecular forces called crosslinks
This holds the chains firmly together
What does LDPE stand for?
Low density poly(ethene)
What does HDPE stand for?
High density poly(ethene)
Why do LDPE and HDPE have different properties?
They are made under different conditions
Properties of LDPE
Polymers have side branches that disrupt the regular arrangement so it has a LOW density
Forces of attraction are weak as chains are further apart
More transparent and flexible then HDPE
Properties of HDPE
Molecules line up so the density is HIGH Molecules are held together strongly so it has a high melting point Forces of attraction are strong Very few, if any side branches Stiff, rigid and strong
What is LDPE used for?
Bags and bottles
What is HDPE used for?
Water tanks and drain pipes
How is LDPE made?
Hearing ethene to 100-300 degrees under high pressure
Oxygen used in reaction
How is HDPE made?
Made at a lower temperature and pressure with a aluminium based metal oxide as a catalyst
Thermosoftening polymers properties
No regular structure
Forces between chains are easy to overcome
Easy to melt
Can be remelted and remoulded as many times as you like
Thermosetting polymers properties
They have cross links which hold it together in a solid structure Strong covalent bonds Doesn't soften when heated Difficult to melt Cannot be remoulded once heated Strong, hard and rigid
Examples of thermosoftening polymers
Plastic bottles
Containers
Examples of thermosetting polymers
Cooking spatulas
Pan handles
Plug sockets
Why are thermosoftening polymers easily separated and can melt?
Weak intermolecular forces
Polymers can separate more easily at lower temperatures so les heat is needed to separate the chains
Define relative atomic mass
How heavy different atoms are compared with the mass of an atom of carbon 12
How can you find the relative atomic mass?
It’s the same as the mass number of the element (top number)
Define relative formula mass (2)
Relative atomic masses added together
OR
The relative formula mass of a substance, in grams is one mole of that substance.
Number of moles formula
Number of moles =
Mass in g of the element/ compound
DIVIDED BY
The relative formula mass of the element/ compound
Percentage mass of an element in a compound formula
Percentage mass = Relative formula mass of element x number of atoms of the element DIVIDED BY Relative formula mass of compound MULTIPLIED BY 100
What is the percentage mass of sodium in sodium carbonate?
23 x 2 divided by 106 times 100 equals
43.4%
How do you find the empirical formula from masses or percentages? (5)
- List all elements given
- Below, write the masses or percentages given
- Divide each mass or percentage by the relative formula mass (masses added together)
- Divide both answers by the smallest answer
- Write out the empirical formula
Empirical formula of carbon and oxygen
- C= 1.2g, O=3.2g
- C=12, O=16
- C= 1.2/12=0.1, O=3.2/16=0.2
- C= 1.2/1.2=1, O=0.2/0.1=2
- CO2
How do you calculate masses in a reaction?
- Write out the balanced equation
- Work out the relative formula mass (for the two bits you need)
- Divide to get one, then multiply to get all (do this on both sides)
Percentage yield formula
Percentage yield = actual yield (grams) DIVIDED BY predicted yield (grams) TIMES BY 100
What is a percentage yield?
Tells you the overall success of an experiment
It compares the predicted yield and the actual yield
What is yield?
The amount of product you get from a reaction
The more reactants you start with, the … the actual yield
Higher
What doesn’t yield percentage depend on?
The amount of reactants you started with, because it is a percentage
How can the predicted yield of a reaction be calculated?
Using the balanced equation reaction
Predicted yield can also be known as the …
Theoretical yield
What percentages are percentage yield in between?
0-100%
What does a 100% yield percentage suggest?
You got all the product you expected to get
What does a 0% percentage yield suggest?
No reactants were converted into a product, so no product was made
Why can you never get a 100% yield percentage?
Some product or reactant will always get lost along the way (including big industrial processes as well as school lab experiments)
Why can product and reactants get lost along the way?
- Reversible reactions
- Filtration
- Unexpected reactions
How can reversible reactions lead to product/reactant being lost?
Reactants will never be completely converted to products as the reactions goes both ways, which results in a lower yield
How can filtration lead to product/reactant being lost?
When you filter a liquid to remove solid parts, you always lose a bit as it may get separated from the reaction mixture
How can unexpected reactions lead to product/reactants being lost?
Unexpected reactions may use up reactants, so there is not as much reactants to make the product you want
What is a reversible reaction?
Where the products of the reaction can react with themselves to product the original reactants
What is an example of a reversible reaction?
Ammonium chloride ammonia + hydrogen chloride
What is sustainable development about?
Making sure we don’t use resources faster than we can replace them
Why is the highest product yield sustainable?
It uses little energy
Resources are saved
Why is a low yield not as sustainable?
Chemicals are wasted
How can you tell which dye is the most soluble?
It will move furthest up the paper
What is paper chromatography used for?
Separating artificial colours such as food colouring (containing one dye or a mixture of dyes)
How does paper chromatography work?
- Extract the sample into a cup with water
- Draw a pencil baseline on some filter paper and add spots of the coloured solution
- Add the paper into the water, making sure the pencil like is above the solution
- Different dyes will then form onto the paper
What does a chromatogram with four spots suggest?
At least four dyes, not exactly four dyes
What is gas chromatography used for?
Separating a mixture of compounds and helping to identify the substances present
How does gas chromatography work?
- A carried gas carries substances through a column with solid material
- the substances travel and different speeds so they are separated
- the detector helps to identify the substances
- a recorder then draws a gas chromatograph
What is the retention time?
The time it takes for the substances to reach the detector
What does the number of peaks in a gas chromatograph show you?
The number of different compounds in the sample
What does the position of the peaks in a gas chromatograph show you?
The retention time of each substance
What is GC-MS?
When the gas chromatography column is linked to a mass spectrometer.
It identifies the substances leaving the column QUICKY and ACCURATELY
How do you work or the relative formula mass of the substances from a GC-MS?
Read it from the molecular ion peak on the graph it draws
the peak furthest to the right
Advantages of using machines to analyse unknown substances (3)
- sensitive
- fast
- accurate
Paper chromatography - summary
Paper - Mobile phase is liquid Analyse food dyes Stationary phase is paper Easy to do Difficult to obtain accurate results Substances travel at different speeds Analyse mixtures in a solution
Gas chromatography - summary
Gas - Mobile phase is gas Used to detect alcohol in breath Stationary phase is a solid packed in a column Requires special equipment Gives accurate results Substances travel at different speeds Analyse substances in a vapour Sensitive
Example of a slow reaction
The rusting of iron
Example of a moderate speed reaction
Metal reacting with an acid
Example of a fast reaction
An explosion
What does a rate of reaction depend on? (4)
- Temperature
- Concentration (or pressure for gases)
- Catalyst
- Surface area of solid
How can the rate of reaction be observed? (2)
How quickly the reacts are used up
How quickly the products are formed
Formula to calculate rate of reaction
Rate of reaction=
Amount of reactant used/product formed
DIVIDED BY
time
Ways the rate of reaction can be measured (3)
Precipitation
Change in mass (usually a gas given off)
Volume of gas given off
How can the rate of reaction be measured precipitation?
This is when the product is a precipitate and makes the solution go cloudy
You can observe a mark in the solution to see how long it takes for it to disappear
The quicker it disappears, the quicker the reaction
People may disagree to when the “mark” disappears
How can the rate of reaction be measured by a change in mass?
This can be carried out on a mass balance
As the gas is released, the mass disappearing is measured on the balance
The quicker the reading drops, the faster the reaction
Most accurate
However, the gas gets released straight into the room and if the flask is too hot, mass may be lost by evaporation
How can the rate of reaction be measured by the volume of gas given off?
This involves a gas syringe
The more gas given off in a certain time interval, the faster the reaction
Mostly accurate results
If the reaction is too vigorous, the plunger may blow out of the syringe
What is the collision theory?
The theory that the rate of reaction depends on how often and how hard particles collide with each other
How does temperature increase collisions?
As temperature increases gain more kinetic energy
Therefore they move faster
Causing more successful collisions
How does concentration/pressure increase collisions?
A higher concentration/pressure means more particles are squashed together
Therefore they are more likely to collide as there is less free space
So there are more frequent collisions
How does surface area increase collisions?
A larger surface area means there is more area for the particles to react with
So there is more frequent collisions
How does a catalyst increase collisions?
A catalyst provides a surface for reacting particles to stick to
Which increases the number of successful collisions
What is a catalyst?
A substance that speeds up a reaction without being changed or used up
What is the activation energy?
The minimum amount of energy required for particles to react
Advantages of catalysts
Used in many industrial reactions
Saves money
Allows reactions to work at lower temperatures saving energy
Can be reused
Disadvantages of catalysts
Expensive to buy and clean
Different catalysts are required for different reactions
Can stop working by impurities
What is an exothermic reaction?
When (heat) energy is transferred to the surrounding and is shown by a rise in temperature
Examples of exothermic reactions (3)
- burning fuels e.g combustion
- neutralisation reactions
- oxidation reactions
- everyday uses e.g hand warmers
What is an endothermic reaction?
Takes in (heat) energy from surroundings and is shown by a fall in temperature
Examples of endothermic reactions (2)
- thermal decomposition
- everyday uses e.g injury ice packs
Define anyhydrous
Without water
Define hydrated
With water
In reversible reactions why are they endothermic in one direction and exothermic in the other?
The energy absorbed by the endothermic reaction is equal to the energy released
What is the pH scale?
A measure of how acidic or alkaline a solution is
What would the pH of the strongest acid be?
0
What would the pH of the strongest alkaline be?
14
What does a pH of 7 suggest?
It is neutral, e.g pure water
How can you estimate the pH of a solution?
Using an indicator
How does universal indicator work?
It changes colour depending on whether it is above or below a particular pH
(s)
Solid
(l)
Liquid
(g)
Gas
(aq)
Dissolved in water
What is an acid?
An acid is a substance with a pH of less than 7
What ions do acids form in water?
They form H+ ions which make solutions acidic
What is an Alkali?
An alkali is a base that dissolves in water
What is a base?
A substance with a pH of above 7
What ions do alkalis form in water?
They form OH- ions that make solutions alkali
What is the reactions between acid and bases called?
A neutralisation reaction
What is the equation for a neutralisation reaction?
acid + base -> salt + water
What is the equation for a neutralisation reaction in terms of ions?
H+ (aq) + OH- (aq) -> H20 (l)
If a substance is neutral what colour will the indicator turn?
Green
What is the equation for the reaction of an acid and metal?
Acid + metal -> salt + hydrogen
How does the reactivity of a metal affect the rate of the reaction?
The more reactive the metal, the faster the reaction will be
Why does copper not react with dilute acids?
It is less reactive than hydrogen
In reactions of metal and acid, how can the speed be measured?
The rate at which bubbles of hydrogen are given off
What is the burning splint test?
The test for hydrogen which can be identified by placing a burning splint into the solution and hearing a squeaky pop
What does the name of the salt produced depend on?
The metal and acid used
Hydrochloric acid will produce which salts?
Chloride
E.g. magnesium chloride
Sulfuric acid will always produce which salts?
Sulfates
E.g Zinc sulfate
What is the reaction of an acid and metal oxide?
Acid + metal oxide -> salt + water (neutralisation reaction)
What is the reaction of an acid and metal hydroxide?
Acid + metal hydroxide -> salt and water (neutralisation reaction)
When ammonia dissolves in water what is the product?
An Alkaline solution
Reaction of ammonia and nitric acid equation
Ammonia + nitric acid -> ammonium nitrate
NH3 (aq) + HNO3 (aq) -> NH4NO3 (aq)
Why is the reaction of ammonia and nitric acid different to other neutralisation reactions?
There is NO water produced, only three ammonium salt
Why is ammonium nitrate a good fertiliser?
It has nitrogen from the ammonia and the nitric acid which plants require to make proteins
Which salts are soluble in water?
Most chlorides, sulfates and nitrates
Except lead chloride, lead sulfate and silver chloride
Which salts are insoluble in water?
Most oxides and hydroxides
How to make SOLUBLE salts with a metal/insoluble base
- Pick the correct acid and base/insoluble salt
- Add the metal, metal oxide or hydroxide to the acid which should then dissolve as it reacts.
- The acid has been neutralised when excess solid sinks to the bottom
- Filter out the excess solid parts to leave the salt solution
- For pure crystals, evaporate some of the water to make it more concentrated and leave to evaporate (crystallisation)
How to make SOLUBLE salts using an alkali
Acid + alkali -> salt + water
- Use universal indicator to mix and see when the reaction is finished and measure the amount you have used
- Repeat without the indicator so the salt is not contaminated with indicator
- Evaporate and crystallise
How to make INSOLUBLE salts using a precipitation reaction
Pick two solutions that contain the ions you need
Mix them together
Once the salt is precipitated, it will sink to the bottom
Filter the solution, wash and then dry it on filter paper
What are precipitation reactions used for?(2)
- To remove poisonous ions e.g lead from drinking water
- To treat effluent (sewage) and removed unwanted ions
What is electrolysis?
Passing an electric current through an ionic substance (that’s molten or in solution) to break it down into the elements it’s made up of
What is the electrolyte?
The liquid required to conduct the electricity
Why does electrolysis only occur in molten or dissolved ionic substances?
As electrolytes contain free ions that allow electricity to be conducted
Where do electrons move to during electrolysis?
Electrons are taken away from ions at the positive electrode and move the to the negative electrode
What do ions become when the lose or gain electrons?
Atoms or molecules
OIL RIG
Oxidation is losing electrons
(and gaining oxygen)
Reduction is gaining electrons
(and losing oxygen)
Electrolysis of molten lead bromide
- Lead is produces at the negative electrode (Reduction)
- Bromine is produced at the positive electrode (Oxidation)
- At the negative electrode, one lead ion accepts 2 electrons and becomes one lead atom
- At the positive electrode, two bromide ions lose one electron each to become one bromine molecule
What can affect the products formed by electrolysis?
The reactivity series of metals
How does the reactivity of metals affect products at the negative electrode?
Hydrogen js produced unless the metal is less reactive than hydrogen
This is because more reactive ions want to stay within the solution
How does the reactivity of metals affect products at the positive electrode?
If OH- and halide ions (Cl-, Br, l-) are present then one of the halide ions will form.
If no halide is present, oxygen will be formed
What are the products when sodium chloride solution is electrolysed? (3)
Hydrogen
Chlorine
Sodium hydroxide
Electrolysis of sodium chloride solution
- At the negative electrode, two hydrogen ions accept 2 electrons to become one hydrogen molecule
- At the positive ions, two chloride ions lose their electrons to become one chlorine molecule
- Sodium ions remain in solution as they are more reactive than hydrogen, and hydroxide ions from the water are left behind. Therefore sodium hydroxide is left in the solution.
Half equations for electrolysis of molten lead bromide
Negative electrode: Pb2+ + 2e- —> Pb
Positive electrode: 2Br- —> Br2 + 2e-
Half equations for electrolysis or sodium chloride solution
Negative electrode: 2H+ + 2e- —> H2
Positive electrode:
2Cl- —> Cl2 + 2e-
OR
2Cl- - 2e- —> Cl2
Products from the electrolysis of sodium chloride solution
- Chlorine can be used in the production of bleach and plastics
- Sodium hydroxide is a strong alkali and is therefore used to make soap
Why is electrolysis used with aluminium?
It is used to remove aluminium (found naturally in compounds) from its ore which is bauxite
After mining and purifying, pure aluminium oxide is left (a white powder), so the aluminium gets extracted through electrolysis
Why is cryolite used in the electrolysis of aluminium
Aluminium oxide has a high MP (over 2000 degrees) so melting would be expensive
Instead dissolving it in molten cryolite would bring the temperate down to 900 degrees
This makes it cheaper and easier
Why are electrodes in the electrolysis of aluminium made of carbon?
It is a good conductor of electricity
Electrolysis of aluminium
Aluminium forms at the negative electrode
Oxygen forms at the positive electrode
At the positive electrode, carbon dioxide can get formed because the oxygen reacts with the carbon, therefore the positive electrodes have to get replaced as they can get eroded
Half equations for the electrolysis of aluminium
Negative electrode:
Al3+ + 3e- —> Al
Positive electrode:
202- —> O2 + 4e-
What is electroplating?
Electroplating used electrolysis to coat the surface of one metal with another
Uses of electroplating
Decoration - silver is attractive but expensive so it’s character to plate a brass cup with silver instead
Conduction - metals like copper conduct electricity well so they’re used to plays metals for circuits and computers
In electroplating what is at each electrode, and what is the electrolyte?
The negative electrode is the metal object you want to plate
The positive electrode is the pure metal you want it to be plated with
The electrolyte must contain a solution containing the ions of the plating metal
Electroplating of silver onto brass
Brass would be the negative electrode
A lump of pure silver would be the positive electrode
The electrolyte would be silver nitrate (as it includes silver ions)
Rate of reaction experiments (4)
HCL acid and marble chips
Magnesium and dilute HCL
Sodium Thiosulfate and HCL
Hydrogen peroxide
Explain the reaction of sodium thiosulfate and HCL
Both clear solutions
React to form a yellow precipitate (sulfur)
Time how long it takes for a black mark to no longer be seen as the sulfur turns cloudy
Repeat for different temps/concentrations
Use hot water bath so acid is not directly heated
Explain the decomposition of hydrogen peroxide
Shows the effect of different catalysts The decomposition is usually quite slow Manganese oxide catalyst speeds it up ( Or catalysts in potato peel/blood ) Oxygen is given off and if used to measure the rate of reaction using a gas syringe 2H202 (aq) ---> 2H20 (l) + O2 (g)
