gcse science chemistry unit C5 cards
- Created by: charlie
- Created on: 08-06-13 17:18
the mole
- 6.023x10^23
- one mole of atoms/ molecules of a sustance will have a mass in grams equal to Ar/Mr
- e.g Carbon Ar 12 + carbon dioxide Mr 44
- formula for finding no. of moles:
relative masses are masses compared to carbon-12:
- relative atomic mass is compared to 1/12th the mass of an atom of carbon-12 (isotope of carbon)
reacting masses + empirical formulas
use ratios or moles to calculate masses in reacting
- 1)write out balanced euqation+ calculate no. of moles in the desired mass of element
- 2)look at the ratio + calculate the mass from the moles
calculating % composition by mass of compounds:
empirical formulas- simplest ratio of atoms in compound
finding it from given masses+elements
- 1)list all elements in compound
- 2)underneath write masses being used in experiment
- 3)divide each mass by Ar for particular element
- 4)turn numbers into simple ratio by multiplying/dividing
- 5)get ratio in simplest from- giving you empirical fromula
concentration
- measure of how crowded things are (moles per dm^3)
- the more solute dissolved the more crowded solute molecules+the more concen.
- 1dm^3=1 litre
calculating concen.
e.g. whats the concen. of a solution with 2 moles of salt in 500cm^3?
converting moles per dm^3 to grams per dm^3
e.g. you have solution of sulphuric acid of 0.04mol/dm^3 what is the concen. in grams per dm^3?
concentration
given concentrated solution+ asked to dilute it to weaken solution
e.g. produce 500cm^3 of 0.1 mol/dm^3 solution of KOH if you're given 1.0 mol/dm^3 solution of KOH + water?
- 1) work out ratios of two concen. - divide to get no. less than 1
- 2) multiply ratio by vol. of solution you want to end up with- tells you how much of original acid tou need to dilute
- 3) work out vol. of water you will need
GDA's are rought estimates
- amounts given in 100g + might eat more or less of product
- may add other things- milk to cereals
using sodium content to estimate salt
e.g. slice of bread contains 0.2g sodium- how much salt does it contain?
- 1) find ratio of sodium chlorides Mr to sodiums Ar
- 2) multiply this by amount of sodium
- wont all come from sodium as may be other compounds- sodium nitrate (preservative)
titrations
- used to find out concen.+exactly how much acid needed to neutralise alkali (vice versa)
- use pipette+pipette filler to add alkali+indicator, fill burette with acid, at eye level add drops of acid swirling after every few drops-when end-point reached(indicator changes colour)
- first experiment is rough idea of how much needed- then repeat to spot anomalies
use single indicators- universal indicators shows range of colour+only rought end point
- phenolphthalein- clear (alkalis) to pink (acid)
- litmus- blue (alkalis) red (acids)
pH curves show pH against vol.- sudden change in pH gives S-shape
calculate concen.-
e.g. start with 25cm^3 of NaOH +concen. is 0.1 moles/dm^3 takes 49cm^3 to neutralise what is concen of the acid?
gas volumes
collection methods depends on gas:
- 1) gas syringe- any gas to nearest cm^3 (quite accurate) but delicate
- 2) upturned m. cyclinder/burette- bubble gas into water, no good for hydrogen chloride or ammonia as they dissolve, burette measures to 0.1 m^3 (accurate)
- 3)mass of gas produced- gas released mass dispering easily recorded- releases gas straight into room but is most accurate
one mole of gas occupies 24 dm^3 at room temp (25d.c)+ pressure (1 atmosphere)
following reactions
reactions stop when one reactant is used up:
- used up reactant= limiting reactant + other reactants are in excess
- amount of product is directly proportional to amount of limiting reactant
faster rates of reaction shown by steeper curves
- when lines reach same amount of product it means they have same amount of limiting reactant
- more limiting reactant makes reaction faster+more product
equilibrium
reversible reaction- where products of reaction can react themselves to produce original reactants
reversible reactions reach equilibrium:
- start- forward reaction falls as reactants turn to products then backward reaction inc. as products turn back into reactants
- eventually forward+backward goes at same rate- reached equilibrium
- only takes place in closed system+concen. of reactant+products are equal +wont change
position of equilibrium can be right or left:
- lie to right- lots of products not much reactants (concen. of product greater than reactant)
- lie to left- lots of reactants not much products
exact postion depends on conditions
- temp
- pressure- only involving gases
- concen.
- *catalyst-- doesnt change e postion- speeds up forwar+backward reaction same amount - makes quicker but still end up with same amount of product
changing equilibrium
equilibrium tries to minimise changes made:
- temp- all reactions exo. in one direction + endo. in the other
- dec. temp - e moves in exothermic direction to produce more heat (vice versa) lies with what is causing exothermic reaction
- pressure- only with gases- inc pressure move in direction where fewer moles of gase (vice versa)
- concen.- inc. concen. by adding more reactants- e tries to reduce shifting to right to produce more products (vice versa)
the contact process
used to make sulphuric acid:
- 1) sulphur(s) + oxygen(g) = sulphur dioxide(g)
- 2)sulphur dioxide(g) + oxygen = sulphur trioxide(g) (reversible reaction)
- 3)sulhur trioxide(g) + water = sulphuric acid
conditions in stage 2 carefully chose as reversible
- temp-exothermic- think that reducing temp will shift e to right inc. heat+products but instead slows reaction down- temp is compromised at 450d.c for quite high yield
- pressure- two moles product three moles reactant- inc. pressure e shifts to right t oreduce pressure+inc. product- expensive + e already on right so only 1 atmospheres used
- catalyst- increase rate (vanadium pentoxide)- doesnt affect position of e
good yield of around 99% of SO3
strong + weak acids
acids produce protons in water- ionise+ produce hydrogen ions
strong acids(sulphuric,hydrochloric,nitric)-
- ionise completely in water- every H2 atoms releases H+
- HCL=H+ + CL-
weak acids(ethanoic,citric,carbonic)-
- dont fully ionise- only some H2 atoms release H+
- CH3COOH=H+ + CH3COO- (reversible reaction)- equilibrium lies well to left
- lower concen. of ions means less charge can be carried
strong acids= what proportion of acid molecules ionise in water
concentrated acids=how many mole/dm^3 of acid(how watered down acid is)-total no. of dissolved
more on strong + weak acids
strong+weak acids react with carbonates in the same way:
- both react with magnesium to give hydrogen
- both react with calcium carbonate to give carbon dioxide
diference between reactions is the rate
- weak acid slower due to equilibrium- releases few H+ ions so add Mg or CaCO+ collision frequency is low, when H+ react concen. dec. so e shifts to left so more H+ ions releases + so on
- stong acid all acid molecules ionised+ H+ ions fully disassociate- so high collision frequency
vol. of gas produced depends on amount of acid:
- rate of reaction is diff. but amount of product is the same- starting with same amount+concen.
- as concen. the same no. of molecules in litre will be the same + each can only let go of 1 H+ therefore total vol. of H2 gas will be he same
precipitation reactions
- involve ions- to react ions need to move + collide
- so therefore ionic substance has to be molten or in solution- really quick reaction as high collison frequency
ionic equations show the useful bits:
- precip. reaction- start with 2 solutions (aq) + end up with a solid (s)
- spectator ions= ions that dont change in the reaction- dissolved before + still afterwards
- ionic equations ignore the spectator ions
testing for sulphate ions
- add dilute HCL then barium chloride
- white precip. of barium chloride means original compound was sulphate
testing for halide ions
- add dilute nitric acid then lead nitrate
- chloride gives white precip. of lead chloride
- bromide gives cream precip. of lead bromide
- iodide gives yellow precip. of lead iodide
preparing insoluble salts
picking right reactants
- e.g. making lead iodide need lead ions + iodide ions + need to be in solution so cant move out
- nitrates soluble so used solution of lead nitrate + can get iodide ions from potassium iodide
- mix ingredients togeth gives a salt (precip reaction)
then... precipitate, filter, rinse, dry... (use distilled water as contains no other ions)
- precipitate(mix) solutions in small beaker with distilled water so ions dissolve- salt precips out
- fliter- using filter paper+funnel stick in concical flask+ pour beaker contents into it+rinse beaker with distilled water + do it again making sure all product is gone
- rinse content with distilled water making sure all soluble salts washed away
- scrape onto fresh filter paper+leave to dry
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