1.02 Quantitative Chemistry

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  • Created by: fs20/22
  • Created on: 05-11-20 12:30

Mass

  • The relative molecular mass of an element is the average mass of an atom of the element compared to 1/12 the mass of a Carbon-12 atom.
  • The relative formula mass of a compound is the average mass of a molecule of the compound compared to 1/12 the mass of a Carbon-12 atom.                                                   
  • The molar mass of a substance is the mass, in grams, of one mole of a substance (= RAM, units = g/mol or gmol-1).
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Moles

mole of substance is the amount of substance which contains as many particles (atoms, ions or molecules) as 12.0g of Carbon-12. 

The number of particles in one mole is 6.02 x 1023, this is Avogadro's constant (L). 

e.g. 1 mole of H2O contains 6.02 x 1023 molecules and therefore 18.06 x 1023 atoms . 

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Mole Calculations 

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Empirical and Molecular Formula

The empirical formula of a compound is the simplest whole number ratio of atoms in a compound. 

The molecular formula of a compound is the actual whole number ratio of atoms in a compound. 

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Concentration (Molarity)

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Back Titrations

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Ideal Gas Equation

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One mole of gas occupies 0.0224 m3 ( 22.4 dm3) at standard pressure (0°C / 298 K and 100kPa / 100,000 Pa). 

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Percentage yield

Percentage yield is a comparison between the amount of product that should form during a reaction and the amount that actually forms. 

  • The higher the percentage yield, the more efficient the reaction is.
  • Percentage yield can never be greater than 100%.
  • Reversible reactions in closed system never reach 100% yield. 

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Atom Economy

Atom economy is a measure of the proportion of reactant atoms that become part of the desired product (rather than by-products) in the balanced chemical equation. 

The higher the atom economy, the less wasteful the reaction. Therefore, companies in the chemical industry will often choose to use reactions with high atom economies. These reactions have economic, environmental and ethical benefits. 

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