Unit 5 - Formulae, Equations and Amounts of Substance (9CH0)
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Summary - Unit 5 - Formulae, Equations and Amounts of Substance (9CH0)
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Unit 5 - Formulae, Equations and Amounts of Substance (9CH0)
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PEARSON (PEARSON)
A summary of topic 5, organised so the notes are easy to understand. The notes are on slides, so they can be printed out and used as revision cards or posters, for revision on the go. The notes cross-reference the specification so it is easy to see where each bit of information has come from. They ...
Unit 5 - Formulae, Equations and Amounts of Substance (9CH0)
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Naming Ionic eq’s:
- IDE = 2 elements 1. Balance
- ATE = 2 elements + oxygen 2. Everything aq split into ions
Common transition metal valencies: 3. Remove spectator ions
Percentage calculations:
% yield = actual yield _ x100
Empirical formula vs molecular formula: theoretical yield
Emp = relative number of atoms of each element present % atom economy = mass of atoms in desired product
Molec = actual number of atoms of each element present x100
To calc molec: mass of atoms in all reactants OR all products
1. Find emp formula % uncertainty = uncertainty of equipment x100
2. Find Mr of emp size of measurement
3. Mr given of molec formule / Mr of emp
4. Emp formula X number from 3. KEY DEFINITIONS
Important equations: Mole = is the amount of substance that contains the same
n = m/Mr number of particles as there are atoms in 12.0 g of carbon-12
n = particles/L L = 6.02 x 10^23 cm^3 →/10^3→dm^3 Molar mass (Mr) = mass of 1 mole of a substance in g/mol
n=cxv dm^3 →x10^3→cm^3
OR mass = c x v dm^3 →/10^3→m^3
Conc = moles/volume (mol/dm^3) mol/dm^3 →xMr→g/dm^3
Conc = mass/volume (g/dm^3) g/dm^3 →/Mr→mol/dm^3
Density = mass/volume (kg/m^3)
Moles = vol(dm^3)/24 or vol(cm^3)/24000
⤷ in gases, Ar = 4g/mol →4g takes up 24dm^3 of space
1 mole of gas takes up 24dm^3 of space at RTP
Ideal gas equation:
2 assumptions:
5. Ideal gas molecules don’t attracts or repel one another
6. Gas molecules themselves take up no volume
PV=nRT T = absolute temp (k)
⤷ kPa = dm^3 R = 8.314J/mol k
⤷ Pa = m^3 n = moles of gas
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