3.1.2 Amount Of Substance Flashcards
Sulfate
SO4²-
Nitrate
NO3-
Nitrite
NO2-
Phosphate
Po4³-
Carbonate
CO3²-
Hydrogencarbonate
HCO3-
Hydroxide
OH-
Magnate(VII)
MnO4-
Chromate (VI)
CrO4²-
Dichromate
Cr2O7²-
Ethanedionate
C2O4²-
Ammonium
NH4+
Silver
Ag+
Zinc
Zn²+
Cyonides
-CN group
Ionic equations
Only ionic compounds(aquous) get split into ions
Then remove any spectator ions
Atom ecpnomy
Ratio of mass of useful product to mass of total reactants (expressed as percentage)
Mr of useful/Mr of reactants ×100
Avogardos equation
Moles×L= molecules
L=6.02×10²³
Empirical Formlae
Represents simplistic whole number ratio of atoms in compound
(Find moles then turn into estimated whole number ratio)
Molecular Formulae
Actual number of atom of each element in one molecule of the compound
Actual Mr/impirical Mr gives multiplier
Ideal Gas Equation
PV=nRT
calculate masses in Combustion Reactions
- find moles of CO2 and H20
-convert to grams to find mass of oxygen in compound
-then find empirical formulae
OR - find mole ratio of Carbon and Hydrogen
-guess the formulae from Mr
Boyle’s Law
while Temp is constant
volume is inversely proportianal to to pressure
Charles’s Law
at constant Pressure
Volume is directly proportianal to Temprature
Absolute 0
0Kelvin
or -273 Celcius