CHEM1201 Lecture Notes - Lecture 3: Molar Mass, Bayerischer Rundfunk, Bromine
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7 Jun 2018
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Steps to calculate molar mass
1. How many atoms of each type are in the compound?
2. What is the atomic mass of each atom in the compound?
3. What is the sum of the atomic masses for the compound?
n = m/M = mass/molar mass
Relating moles and number of atoms
1 mole contains 6.022 x 1023
- How many atoms in 0.25 mole Fe?
o 1.51 x 1023 atoms
- How many atoms in 0.25 mole of water?
o
Elemental formulae
- most elements are composed of single atoms
o e.g. sodium (Na) a highly reactive solid metal
- some elements exist as diatomic molecules
o e.g. chlorine (Cl2) a coloured gas
o Hydrogen H2
o Nitrogen N2
o Oxygen O2
o Fluorine F2
o Chlorine Cl2
o Bromine Br2
o Iodine I2
- Other eleets that are’t ooatoic
o Sulphur (S8)
o Phosphorus (P4) (tetrahedral)
Describing chemical reactions – equations
- Need accurate formulae for
o Reactants
o Products
- E.g. sodium+ chlorine→ sodium chloride
- Na(s) + Cl2(g → 2NaCl(s)
Balancing a combustion reaction
Combustion reactions of a hydrocarbon
1. hydrocarbon reacts with oxygen to produce carbon dioxide and water
2. formulae correct for reactants and products
3. count all the atoms of each side of the arrow (balance)
- CH4 + O2 → CO2 + H2O
- CH4 + 4O2 → CO2 + 2H2O
-
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