Topic 1 Quantitative Chemsitry

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Mind Map on Topic 1 Quantitative Chemsitry, created by kevin86604 on 05/21/2014.
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Mind Map by kevin86604, updated more than 1 year ago
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Topic 1 Quantitative Chemsitry
  1. 1.1 The mole concept and Avogadro's constant
    1. Measurements and unites
      1. kg, s, K, m3, Pa or Nm -2
        1. g, min, ˚C cm3, atm
        2. Amount of substance
          1. Element
            1. Atoms
              1. Compound
                1. Moles
                  1. Number of moles(n) =Mass/Molar mass
                    1. A mole is the amount of a substnace which contains the same number of chemical species as there are atoms in exactly 12g of the isotope carbon-12
                    2. Molecular Formula
                      1. Relative molecular mass
                    3. Avogadro's constant
                      1. 6.02 x 10^23 mol -1
                        1. The number of particles per mole
                        2. Example
                          1. Calculate the amount of water, H20, that contains 1.80x 10^24 molecules
                            1. Solution
                              1. n = N/L n= 1.80x 10-24/6.02x 10^23
                                1. n= 2.99 mol
                      2. 1.2 Formulas
                        1. Emperical formula
                          1. It gives the ratio of the atoms of different elements in a compound.
                          2. Molecular formula
                            1. Shows the actual number of atoms of each element present in a molecule
                          3. 1.3 Chemical Equations
                            1. Balancing equations
                              1. Equation: CH3+O2 -> CO2 + H2O
                                1. Balanced Equation: CH4+2O2 -> CO2+2H2O
                            2. 1.4 Mass and gaseous Volume relationships in chemical reactions
                              1. Limiting reactant
                                1. The limiting reactant is the reactant that determines the theoretical yield of product
                                2. Theoretical yield
                                  1. Theoreticall yield is the mass or amount of product produced according to the chemical equation
                                  2. Percentage yield
                                    1. experimental yield/theoretical yield x 100
                                    2. STP= 273K and 101.3 kPa (1atm)
                                      1. For gas: Number of moles (n)= Volume (V) / Molar Volume
                                        1. The ideal gas equation
                                          1. PV=nRT
                                        2. 1.5 Solutions
                                          1. Concentration
                                            1. Example: A solution of sodium hydroxide has a concentration of 8.00g dm-3. What is its concentration in mol dm-3
                                              1. n=m/M M=2.99+1.01+16.00 = 40.00g n=8.00/40.00= 0.200 [NaOH] = n/V = 0.200/1.00 = 0.200 mol dm-3
                                              2. n=n/V
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