Mount of substance
The mole Avogadro's number
1 mole of any substance contain 6.02 1023 atoms molecules
no of particles Avogadro's number x number of moles
The mole solid
is no of moles
myg
The mole solutions
1 no of moles concentration mold m 3 x volume dm3
1 dm 3
6
The mole Ideal gas equation
PV NRT molesigtaesmperature K 298K 250C
ressure tho of constant 8.31 Jk MOL
Pa Volume
M3
2730C O K OC 273 K
Ionic Equations show ions formed in solution and show which particles are
reacting e g H2504 2KOH KzSoa ZHI H2O is not an ion so leave it as it
2Ht 5092 t 2kt 2OH 2kt 5092 ZHI
ancel any ions
that on
appear 24 204 321420
imma
o th sides to form i charges in the final equationmust balance on the
mplestionic equation left and right of equation
these are spectator ions don't get involved in the reaction
can use equations and mole ratio to calculate theoretical yieldof aproduc
Titration used to work out conc of an acid or alkali
steps
acid alkali with known conc in burette
acid alkali with unknown conc but known vol in conical flask
add indicator to conical flask phenolphthalein acid colourless
alkali pink
alkali red
add chemical in burette to conical flask until indicator changescolor
Known as end point add dropbydrop near end point
read how much chemical was added from the burette to neutralis
read bottom of meniscus at eye level
record results to zap and repeat until you have 2 concordan
suits within 0.10cm 3 of each other
Empirical formula simplest whole number ratio of elements in a compoun
divide the masses by the relative atomic mass of the elements to fin
e moles divide all the molesby the smallest number of moles an element tha
present to find simplest whole number ratio
if I given instead of mass use it as mass
to work out molecular formula calculate Mr of empirical formula divid
r of molecular formula by this multiply all atoms in empiricalformulaby
his value
REMEMBER 1 mole of H2O has 2 moles of Hydrogen
e g empiricalformula of hydrocarbon which combustscompletely to
ake 0.8459 of CO2 and 0.173g of H2O 02 70.845 44 0.019 moles of C
20 70.173118 0.0096 71 mole of H2O has 2 moles of H 500.0096 moles of H
as 0.0192moles of H simplestratio 0.019 0.019 1 1 empiricalformula CH
The mole Avogadro's number
1 mole of any substance contain 6.02 1023 atoms molecules
no of particles Avogadro's number x number of moles
The mole solid
is no of moles
myg
The mole solutions
1 no of moles concentration mold m 3 x volume dm3
1 dm 3
6
The mole Ideal gas equation
PV NRT molesigtaesmperature K 298K 250C
ressure tho of constant 8.31 Jk MOL
Pa Volume
M3
2730C O K OC 273 K
Ionic Equations show ions formed in solution and show which particles are
reacting e g H2504 2KOH KzSoa ZHI H2O is not an ion so leave it as it
2Ht 5092 t 2kt 2OH 2kt 5092 ZHI
ancel any ions
that on
appear 24 204 321420
imma
o th sides to form i charges in the final equationmust balance on the
mplestionic equation left and right of equation
these are spectator ions don't get involved in the reaction
can use equations and mole ratio to calculate theoretical yieldof aproduc
Titration used to work out conc of an acid or alkali
steps
acid alkali with known conc in burette
acid alkali with unknown conc but known vol in conical flask
add indicator to conical flask phenolphthalein acid colourless
alkali pink
alkali red
add chemical in burette to conical flask until indicator changescolor
Known as end point add dropbydrop near end point
read how much chemical was added from the burette to neutralis
read bottom of meniscus at eye level
record results to zap and repeat until you have 2 concordan
suits within 0.10cm 3 of each other
Empirical formula simplest whole number ratio of elements in a compoun
divide the masses by the relative atomic mass of the elements to fin
e moles divide all the molesby the smallest number of moles an element tha
present to find simplest whole number ratio
if I given instead of mass use it as mass
to work out molecular formula calculate Mr of empirical formula divid
r of molecular formula by this multiply all atoms in empiricalformulaby
his value
REMEMBER 1 mole of H2O has 2 moles of Hydrogen
e g empiricalformula of hydrocarbon which combustscompletely to
ake 0.8459 of CO2 and 0.173g of H2O 02 70.845 44 0.019 moles of C
20 70.173118 0.0096 71 mole of H2O has 2 moles of H 500.0096 moles of H
as 0.0192moles of H simplestratio 0.019 0.019 1 1 empiricalformula CH
