Paper 2 Collection ✓ Flashcards
Revise SC1 - 7, 9, 17 - 26
SC1a - What are the arrangements of particles in each of the three states?
- Solid: Regular and close together
- Liquid: Random and close together
- Gas: Random and far apart
SC1a - What are the movements of particles in each of the three states?
- Solid: Vibrate around a fixed position
- Liquid: Move around each other
- Gas: Fast in all directions
SC1a - What are the names of the two state changes between solid and liquid?
- S→ L is Melting
- L → S is Freezing
SC1a - What are the names of the two state changes between liquid and gas?
- L→ G Evaporating (and Boiling)
- G → L Condensing
SC1a - What are the names of the two state changes between Gas and Solid?
- G → S Deposition
- S → G Sublimation
- During these processes they do not become liquid
SC1a - What is overcome during melting and boiling?
Forces of attraction between particles
SC1a - In a heating curve, at which points will the line be flat?
During Melting and Boiling [phase changes] as the temperature doesn’t increase while the forces of attraction are overcome.
SC2a - What are the two key features of a pure substance?
The composition:
- Cannot be changed by physical means
- Is the same in all parts of a piece of the substance
SC2a - What is a mixture?
- A mixture contains multiple elements/compounds that aren’t chamically joined together.
- The composition cannot be changed and so it isnt a pure substance.
SC2a - How will the heating curve of a mixture look different to a pure substance and why?
- Instead of straight lines there will be curves.
- This is because there are multiple different elements which will have different melting points.
SC2b - What is filtration?
Using a filter to trap larger insoluble substances from a mixture.
SC2b - What is cystallisation?
- When a solution is evapourated, meaning that the solvent turns to gas leaving behin dthe solute which forms crystals.
- The size of these crystals depend on the time the crystallisation takes
- (Longer time taken = larger crystals)
SC2b - What is a saturated solution and how can this be changed?
- A saturated solution is a solution in which a solvent contains the highest amount of dissolved solute as possible.
- This limit can be increased by increasing the temperature.
SC2b - Descirbe what a risk assesment is and how it is used when crystallising in a lab.
- Identifying and evaluating the hazards and considering ways of reducing the risk of harmful effects.
- In crystallisation this would be indentifying:
- The solution can spit: wearing eye protection and removing from the bunsen burner before the solution is completely evapourated
- You can get burnt from the bunsen burner: keep your hands away from the flames at all times
SC2c - What is paper chromotography?
- A method of speration that involves having a piece of paper with dots of ink slightly dipped in the water (so that the water doesnt reach the pencil line that the ink is one).
- The solvent is called the mobile phase and the paper contains the stationary phase.
- If an ink moves less up the page it is less attracted to the stationary phase.
- Different inks have different levels of attraction to the stationary phase and so will get sperated out at different distances.
SC2c - How do you measure the Rƒ value of an ink?
Rƒ = Distance travelled by spot ÷ Total distance travelled by solvent
SC2c - What can paper chromotography be used for?
- Distinguishing between pure/impure substances
- Identifying substances by comparing their chromotogram with known substances
- Identifying substances by calculating their Rƒ value
SC2d - What is simple distillation?
The separation of a liquid from its dissloved solids, by evapourating it and condensing the gas formed.
SC2d - What conditions do the components of the solution have to meet for simple distillation to work?
They have to have boiling points that are at least 25° C apart.
SC2d - Describe a simple distillation set-up.
- A side-arm flask on a tripod over a bunsen burner.
- It contains the solution and anti-bumping granules to help the liquid boil more smoothly.
- A thermometer is connected to the top.
- A delivery tube, leading to a conical flask, is surrounded with a cooling jacket (condenser) which takes cold water in from the bottom and puts it out at the top.
- The conical flask is in a bath of ice water.
- The bunsen burner is ona heat resistant mat.
SC2d CP - Which two methods can you use to seperate solvents in an ink?
- Paper chromotography
- Simple distillation
SC2e - Why can’t water be purified by distillation on a large scale?
It takes up too much energy.
SC2e - Why can’t tap water be used for chemical analysis?
Tap water contains small amounts of dissolved salts and minerals which may react and alter the resuslts
SC2e - Describe the stages river water goes through before it can be used in homes.
- First, it is screened with a seive to get rid of large objects such as leaves and twigs
- It is then sent to a sedimentation tank where small particles will settle out at the bottom
- The water is then filtered through layers of sand and gravel
- Finally it is treated with chlorine to kill microbes
SC3a - Name the three base rules of atomic theory.
- All matter is made up of atoms
- Atoms cannot be broken down into smaller parts
- Atoms cannot be created or destroyed
SC3a - Names the three subatomic particles as well as their relative mass and charge.
- Protons:
- M: 1
- C +1
- Neutron:
- M: 1
- C Neutral (0)
- Electron:
- M: 1/1835 (negligible)
- C -1
SC3a - Describe the structure of an atom
- Protons and neutrons centred in a nucleus.
- Electrons orbiting outside in electron shells.
SC3b - What did the Rutherford Gold foil test reveal about the space inside atoms?
Atoms are mostly empty spcae
SC3b - What is an atomic number?
The number of protons in an atom. the bottom number on the symbol for an element
SC3b - What is a mass number?
- The number of protons + neutrons in an atom (the mass).
- The top number on the symbol for an element.
SC3c - What is an isotope?
Two atoms (of the same element) with the same atomic number but different mass numbers (amounts of neutrons)
SC3c - What does the symbol Ar stand for and what does it mean?
- Relative Atomic Mass.
- The average mass of the naturally occurring form(s) of an element in relation to a Carbon-12 atom
SC3c - How do you calculate the Ar of an element from the abundance of its isotopes.
(M1 x A1) + (M2 x A2) (etc.) ÷ 100 (M=Mass A=Abundance)
SC3c - Why does chlorine have a mass number with a decimal?
- It is its relative mass.
- There are two isotopes of chlorine, 35 and 37.
- Chlorine - 35 is more abundant than 37.
SC4a - How did Medeleev organise his periodic table?
By increasing atomic mass
SC4a - What two things did Mendeleev do to the order of elements in his table that made it more sucessful than others?
- Left gaps for certain elements
- Swapped elements around
- He did this because he realised a trend in the chemical and physical properties in relation to the groups of elements
SC4a - How did Mendeleev predict the property of elements such as eka-alluminium (now known as gallium)
He identified the trend in properties down a group and used this information to estimate the properties of undiscovered elements
SC4b - Why does (in the modern periodic table) Tellerium come before Iodine despite having a greater mass number?
- Iodine exists mostly as Iodine-127
- Tellerium has many isotopes ranging from Te-126 to Te-130
- This means Tellerium’s Ar is ~128
- This proves one reason why it is more reliable to order elements by increasing atomic number than by mass number
SC4b - How is the atomic number related to energy given off in x-rays when electrons are fired at an element?
- The square root of the energy given off is directly proportionate to the atomic number.
- This realisation proved the idea of protons and that the atomic number is the number of protons in an atom.
SC4b - What are the four main features of the modern periodic table?
- Elements in a period are in order of increasing atomic number
- Elements with similar properties are in the same group
- Non-metals are on the right and metals are on the left
- The Iodine Tellerium pair reversal is explained
SC4c - How do atoms store electrons?
- Atoms have electrons in orbits of electron shells around the nucleus
- The first shell holds up to 2 electrons
- The second and third shell holds up to 8 electrons
SC4c - How do you work out the electron configuration of an element? Use Chlorine (Atomic number 17) as an example
- Atomic number 17 means 17 protons and thus 17 electrons. 1
- 7-2 is 15, 15-8 is 7, 7-8 is a negative number so there are 2 in the first shell,8 in the second and 7 in the third 2.8.7
SC4c - How does the electron configuration of an atom relate to its position on the periodic table in terms of group and period?
- The total amount of electron shells will be the period it is in.
- The number of electrons in its outermost shell is equal to the group that it’s in.
SC5a - When ionically bonding, what happens to:
- Metals
- Non-metals
- Metals loose an electron(s) as they are closer to 0/8 electrons in their outermost shell and so its easier to loose electrons
- Non-metals are closer to 8/8 electrons in theri outermost shell and so it is easier for them to gain electrons
SC5a - What is the type of attraction in an ionic bond?
Electrostatic forces of attraction
SC5b - How do you work out the ionic formula of an atom and a compound?
- An atom’s ionic formula will depend on the numbe rof electrons in its outer shell.
- If it has to loose electrons to gain a full outer shell, it will be positive by that much.
- If it has to gain electrons it will be negative by that much.
- In a compound, the charges of the ionic compound of an element need to cancel out.
- e.g Mg 2+ and O 2+ will form MgO while Na+ and S2+ will form Na2S
SC5b - What is an ionic lattice structure?
When billons of ions are packed together in a regular structure.
SC5b - What are the main 5 polyatomic ions?
- Ammonium, NH4+
- Hydroxide, OH-
- Nitrate, NO3-
- Carbonate, CO32-
- Sulfate, SO42-
SC5c - Are the melting and boiling points of Ionic compounds high/low and why?
They are high as they have strong electrostatic forces of attraction which require a lot of energy to overcome and break
SC5c - Are ionic compounds electrically conductive and why/why not?
For a substance to be conductive it must contain particles that are:
- Charged
- Free to move
So Ionic compounds can conduct electricity when they are aqueous or molten.
SC5a - What is a cation and an anion?
- Cation: A positively charged ion (A metal which has lost an electron) Anion
- A negatively charged ion (A non-metal which has gained an electron)
CAT-ions are PAWS-ative (Thank you Mr. Moore #gonebutnotforgotten)
SC5c - How does an aqueous ionic compound conduct electricity?
The negative ions flow to the anode(+) and the positive ions flow to the cathode(-). electrons do not flow.
SC6a - How do covalent bonds work?
- Two atoms with incomplete outer electron shells, share some electrons so that they each have full shells of electrons.
- For example Hydrogen is missing one electron and Chlorine is missing one and so they bond and have a pair of electrons shared between them.
SC6a - Why do molecular compounds (covalently bonded) have low melting points?
While the electrostatic forces between the atoms in single molecule are very strong, the intermolecular forces of attraction are very weak and so they require little energy to break.
SC6a - What is the valency of an atom and how does this affect the amount of bonds it forms?
- The valency is the number of empty spaces in its outermost shell.
- The valency is equal to the total number of bonds formed.
- When Carbon bonds Sulfur there are two sulfurs to one carbon each with a double bond (sharing two pairs of electrons) S=C=S
- This means each sulfur has a valency of two and the carbon has a valency of four.
SC7a - What is a compound?
Atoms of more than one element joined together by chemical (covalent) bonds
SC7a - Why do simple molecular compounds have low m.p/b.p?
- They are formed of covalent bonds
- While there are strong covalent bonds, the forces between molecules are weak meaning they require little energy to break
SC7a - Why aren’t simple molecular compounds able to conduct electricity?
- For something to be able to conduct electricity it must contain a charged particle that is free to to move.
- Covalent bonds aren’t based on charges tso it doesn’t meet these requirements
SC7a - What are polymers and monomers?
- Monomers are small simple molecules.
- When multiple of these join up in a chain, they form a polymer
SC7b - What are allotropes?
Different structural forms of the same element
SC7b - Describe the structure and properties of a fullerene?
- Fullerenes are spherical or tubular structures where each carbon atom is bonded to three others
- They have low m.p/b.p due to weak intermolecular forces
- They are also soft and slippery
- Can conduct electricity due to delocalised electron
SC7b - Describe the structure and properties of graphene?
- Flat shape that cna be rolled up
- Each carbon atom is bonded to threee others meaning there is a delocalised electron allowing conduction of electricity
- Low m.p/b.p
SC7b - Describe the structure and properties of graphite?
- High melting point due to strong covalent bonds
- Layers easily slide over eachother due to weak forces between them
- Three bonds per carbon atom
- Delocalised electron allows conduction of electricity
- Useful as a lubricant due to layers sliding
- Used for electrolysis as it is unreactive and cheap
SC7b - Describe the structure and properties of diamond?
- Tetrahedral structure
- Four bonds per carbon atom
- Electrical insulatro due to no free electrons
- High melting point due to strong covalent bonds
- Very strong due to tetrahedral structure
- Used for drills due to strength
SC7b - Whare are diamond and graphite examples of?
Giant molecular structures: Huge 3D netwroks of atoms linked by bonds
SC7c - What is metallic bonding?
- Metals are bonded in a giant lattice structure
- They are held together by the stron electrostatic forces of attraction that exist between the positive metal ions and the negative delocalised electons
- Strong electrostatic forces of attraction require a lot of energy to break giving them high m.p/b.p
- Delocalised electron allows it to conduct electricity
- They are also malleabele
SC7c - How are metals malleable?
- Mallebale means that it can change shape and bend without breaking
- Metals are a giant lattice structure of positive metal ions delocalised electrons
- When a force is applied to a metal, the layers slide over each other
- It doesn’t break because of the ‘sea’ of delocalised electrons holding the metal together by electrostatic forces
SC7c - Why are metals able to conduct electricity?
- To be able to conduct electricity, something must contain a charged particle that is free to move
- Since metals have a sea of deloclised electrons, it meets these two requirements
- When a potenital difference is applied, the electrons move to the positive side
SC7c - How does the electrical conductivity of a metal vary?
- As the charge of the ion increases, the number of delocalised electrons per atom increases.
- This increases the electrical conductivity
SC7d - What are the advantages and disadvantages of using dot and cross diagrams?
Pros:
- Shows how electrons are shared in covalent and ionic bonds
Cons:
- Do not show the structure formed
- Suggests that electrons are different
SC7d - What are the advantages and disadvantages of using metallic models?
Pros:
- Shows it is held in a lattice
- Explains properties such as eletical conductivity
Cons:
- Doesn’t show the ions to be constantly vibrating
SC7d - What are the advantages and disadvantages of using 3D ball and stick diagrams?
Pros:
- They show the structure that is formed
- They show the number of bonds per atom
Cons:
- The atoms are too far apart
- There aren’t actually any ‘sticks’
SC9a - What is the difference between emirical and molecular forumla?
- Molecular formula is the actual amount of atoms of each element in a compound
- Empirical formula is the simplest whole number ration of atoms of each element in a compound
SC9a - How do you work out the empirical formul of a compound from the masses of each element?
- Find the moles by doing mass/Mr
- Divide both of the molar values by the smalles of the two
- e.g: 10g of Ca and 17.8g of Cl 10/40 = 0.25 17.8/35.5 = 0.5 0.25/0.25 = 1 0.5/0.25 = 2 1:2 ratio
SC9a - Describe how you can find the empirical formula of magnesium oxide by heating magnesium ribbon.
- Place a tripod over a bunsen burner on a heat resistant mat and place a pipeclay triangle on the tripod
- Sand down the magnesium ribbon and measure its mass
- Meausre the mass of the crucible and lid
- Measure the mass of the crucible with the magnesium in and take away your previous result to get the starting value of magnesium
- Let the magnesium ribbon heat over the bunsen burner in the crucible, lifting the lid occasionally to let in oxygen
- Weight the mass of the crucible with the magnesium oxide and take away the mass of the crucible to find the mass of magnesium oxide
- Take away the mass of magnesium to find the mass of oxygne that reacted
- Use the emirical formula method to use these amsses to sork out empirical formula of MgO
SC9c - What is the molar mass formula?
mol = mass/Mr or Ar (relative atomic or formula mass)
SC9b - how do you work out the concentration of a solution?
Concentration (g dm-³) = mass of solute (g) ÷ volume of solution (dm³)
SC9b - What is a dm³ equal to?
1L = 1000 cm³
SC9b - What is the conservation of mass and what doe sit depend on?
- The idea that the mass of the reactants = the mass of the products in a closed system.
- In an open system, gases and liquids can sometimes ascape altering this
SC9b - How do you calculate the mass of a reactant needed to make a product (or vice versa)
- Work out the mols in the one you’ve been given the mass for and divide this by the big number next to it
- Multiply this my the big number next to the one you are trying to work out to give you the mols in this
- Multiply this by its Mr to get the mass
- Example: 2Al + 3Cl₂ → 2AlCl3
- How many grams of Cl₂ to form 53.4g of AlCl3
- AlCl3 has an Mr of 133.5 so do 53.4 ÷ 133.5 = 0.4
- As the ratio of big number is 3:2 do 0.4 ÷ 2 and then x 3 to get 0.6 Do 0.6 x Cl₂s Ar whcih is 71 to get 42.6g
SC9c - What is avrogodos constant?
The amount of particles in a mole 6.02x1023
SC9c - What iis a limiting reactant?
- When you have the mass of two reactants, one is likely to be in excess meaning that once one is used up the one in excess will stiil have some remaining.
- As once one has been used up the reaction can’t continue, the one that gets used up first is the limiting reactant
SC9c - How do you work out the limiting reactant?
- Firstly work out the balanced equation of the reaction (This may already be given to you)
- The big numbers show the rati of mols needed
- Using the mass and Mr, work out the mols you have of one of them
- From here, work out the mols you need for the other one for the second one to not be the limiting reactant
- Then work out how many mols you have of the second one.
- If it is more than you would’ve needed then it is in excess if not then it is the limitjng reactant
- Use the values for the actual amount of mols used up to figure out the masses that will actually be used up
SC9c - What is stochiometry?
The ratio of moles is a reaction
SC17a - What are the physical properties of the alkali metals (group 1)
- Malleable
- Good conductors of electricity
- Relatively low melting points
- Soft/easily cut
SC17a - Why are alkali metals stored in oil?
They are incredibly reactive and would react with the oxygen and moisture in air otherwise.
SC17a - When you cut an alkali metal, a layer of tarnish forms. What is this called and what is the equation for this?
This is oxidation.
4x(s) + O2(g) -> 2x2O(s) Metal + Oxygen → Metal Oxide
[Where x is any alkali metal]
SC17a - How does the melting point of the alkali metals change as you go down?
It decreases
SC17a - What is the equation for the reaction that takes place when an alkai metal reacts with water?
2x(s) + 2H2O(l) → 2xOH(aq) + H2(g)
SC17a - What would you observe when you put lithium, sodium and potassium in water that contains universal indicator?
- Li: Bubbling fiercely on the surface and moves around a bit. Water turns purple
- Na: Moderate effervesance (fizzing) on the surface. Moves about quicker. Might have a yellow spark. Water turns purple
- K: Lots of effervesance (fizzing) on the surface. Moves about very fast. Lilac flame produced. Water turns purple.
- Effervesance/bubbling indicates the presence of a gas (hydrogen)
- Water turns purple becuase it is alkali.
- Increased speed indicates a higher rate of reaction
SC17a - What happens to the reactivity of alkali metals as you go down?
It increases.
SC17a - The reactivity of alkali metals increases as you go down the table. Explain why this is using Lithium and Potassium as examples.
- Both Lithium and Potassium want to loose their only outer shell electron to gain a full outer shell and become stable
- Potassium has more shells of electrons and so there are more shells between its positive nucleus and its outer most electron
- The shells in between shield the positive charge
- Additionally it is urther away from the nucleus
- The positive charge from Lithium’s outermost electron is shielded by less shells and so the electrostatic forces of attraction to its outer shell electron are stronger
- As Potassium has weaker electrostatic forces of attraction to its outer shell electron, this electron can be los tmore easily
- This means Potassium will be more willing to loose its electron to form an ion making it more reactive.
- Thus as you go down the group, every extra layer of electron shells makes the element more reactive
SC17b - What is the name for group 7 elements and what is key about their natural state?
- The halogens.
- They exist covalently bonded as diatomic atoms.
SC17b - What is fromed when a halogen reacts with a metal (e.g. Chlorine and Magnesium)?
- It forms a halide salt.
- Cl2(g) + Mg(s) → MgCl2(s)
SC17b - What happens to the name of a halogen once it it becomes an ion?
- It changes from -ine to -ide
- e.g. BromiNe atom to BromiDe ion
SC17b - What is the trend in mp/bp and density of halogens as you go down the group?
It increases.
SC17b - What are the appearances of Chlorine, Bromine and Iodine at room temperature?
- Cl: Green gas
- Br: Brown liquid
- I:Purple/grey solid
SC17b - What are the properties of Halogen gases?
- Non-metals
- Diatomic
- Toxic
- Corrosive
- Brittle when solid
- Low mp/bp
- Poor conductors of electricity and heat
- Coloured vapours
SC17b - What is the common use for all the halogens?
As disinfectancs/bleaches as they can kill microorganisms and remove stains.
SC17b - Using Hydrogen and Chlorine as examples explain how halogen gases cna be used to from acidic solutions.
- Hydrogen and a halogen bond to from hydrogen halide.
- This is dissolved in water to from an acidic solution. For example:
- Hydrogen + Chlorine → Hydrogen Chloride
- This can dissolved in water to form Hydrochloric acid
SC17b - What is the test for chlorine?
Damp blue litmus paper will turn red and bleach white in the presence of chlorine gas.
SC17c - What observations will you make when you heat halogens with iron wool and what does this tell you about the reactivity trend?
- Fluorine: Bursts into flames
- Chlorine: Glows brightly
- Bromine: Glows dull red Iodine
- Changes colour
- As the reaction gets less violent as you go down the group you can tell that they get less reactive.
SC17c - What is a displacement reaction?
A reaction in which a more reactive element displaces a less reactive metal from a compound producing the less reactive metal
SC17c - State what observation you would make in each of these reactions signifying that displacement has taken place:
- Fluorine + Potassium chloride
- Chlorine + Potassium bromide
- Bromine + Potassium iodide
- Solution turns yellow showing that chlorine has been produced
- Solution turns orangey-brown showing that bromine has been produced
- Solution turns dark brown showing that iodine has been produced
SC17c - Why is displacement a redox reaction?
- Because both oxidation and reduction occur at the same time.
- e.g 2Cl- + F2 → Cl2 + F-
- The chlorine looses electrons at the same time that the fluorine gains electrons and so it is a redox reaction
SC17c - Using Fluorine and Iodine as examples explain why the reactivity of halogens decreases as you go down the group?
- Both Fluorine and Iodine want to gain one outer shell electron to have a full outer shell and become stable
- Iodine has more shells of electrons and so there are more shells between its positive nucleus and its outer most electron
- The shells in between shield the positive charge
- Additionally it is further away from the nucleus
- The positive charge from Fluorine’s outermost electron is shielded by less shells and so the electrostatic forces of attraction to its outer shell electron are stronger
- As Fluorine has stronger electrostatic forces of attraction to its outer shell electron, the last needed electron is attracted more easily
- This means Fluorine will be more willing to gain an electron to form an ion making it more reactive.
- Thus as you go down the group, every extra layer of electron shells makes the element less reactive as there is more shielding and it’s harder to gain an electron
SC17d - What is another name for the group 0 elements?
Group 8 / Noble gases
SC17d - What are the properties of the noble gases?
- Colourless
- Have very low m.p/b.p
- Poor conductros of heat and electricity
- Inert/unreactive
SC17d - What is the trend in m.p/b.p and density as you go down the group?
It increases
SC17d - Why weren’t the noble gases discovered until the late 19th century?
They don’t form compounds and are in very small amounts in our atmosphere and so are hard to detect.
SC17d - What are the uses for each of the noble gases from helium to krypton?
- He: Used for weather ballons/airships as it is non-flammable and has a low density
- Ne: Used in electrical signs for its orange-red glow when electricity passes through
- Ar: Used in the space above wine to preserve it as its denser than air will stop the wine from reacting
- Kr: Used in photography lighting for its brilliant white light when electricity passes through
SC17d - Describe, in terms of their electron configuration, why halogen gases are inert?
- Halogen gases have complete outer shells (e.g. 2 in helium or 8 in neon).
- This means that they are stable as their energy levels are full.
- Thus they ahve no need to loose any electrons.
SC17d - Explain why, despite being a halogen gas, Xenon can still form compounds?
- Xenon has many shells of electrons.
- These shield the positive charge form the nucleus meaning that the positive electrostatic force of attraction acting on its outer layer is weaker.
- Thus if it is near to an atom with few shells (such as fluorine) and is close to the positive charge from that nucleus, the elctron may transfer over.
SC18a - What is the rate of a reaction?
The speed at which reactants turn into products
SC18a - How can you use a gas syringe to investigate the rate of reaction?
- Works for reactions where a gas is produced
- Set up a liquid in a conical flask
- Push a gas syringe to 0 and attach it to a bung
- Add the granules of the other chemical into the conical flask and immediately attach the bung
- Also set off a timer. Every 10 seconds record down the value red on your gas syringe
- Repeat and take the average of concordant results
- use the average results and plot them on a graph
SC18a - Describe a reactant/product time graph showing the rate of reaction
- Concentration on y axis time on the x axis
- Products start at 0 and have an increasing positive curve
- Reactants start high and have an increasing positive curve till 0
- Both curves will plateau (flatten out) at the same point
SC18a - How can you measure mass to investigate the rate of reaction?
- Work for reactions where one of the products are gases
- Place the conical flask on the balance at set it to 0
- Add the liquid being used into the conical flask and then add the other chemical
- Quickly record down the starting mass and cover the flask with cotton wool to stop acid form spitting
- Set off timer and record down the mass every 10 seconds
- Repeat and take the average of concordant results
- Plot a graph using the average results
SC18b - What are the five main factors that affect rates of reaction?
- Temperature
- Pressure
- Concentration
- Surface areas/volume ratio
- Presence of a catalyst
SC18b - How does temperature affect the rate of reaction?
- An increase in temperature gives the reactant particles more kinetic energy meaning they move around more
- This means there will be more frequent successful collisions and more particles will have the required level of energy to react
SC18b - What is activation energy?
The minimum amount of energy required for a reaction to occur
SC18b - How does concentration affect the rate of reaction?
- An increase in concentration means more particles in a fixed volume
- This means that that successful collisions will be more frequent as particles are closer together
SC18b - How does pressure affect the rate of reaction?
- An increase in pressure means the same amount of particles in a smaller volume
- This means that that successful collisions will be more frequent as particles are closer together
SC18b - How does surface area/volume ratio affect the rate of reaction?
- An increase of the surface area to volume ration means for a fixed volume, there is more surface area.
- This leaves more of the surface exposed
- This means that collisions have more surface to occur on and so successful ones occur more often