quantitative chemistry (c3)

    Cards (39)

    • Law of conservation of mass
      No atoms are lost or made during a chemical reaction so the mass of the products = mass of the reactants
    • Balanced chemical equation
      • The numbers of atoms of each element involved are the same on both sides of the equation
    • Relative formula mass (Mr)

      Sum of the relative atomic masses of the atoms in the numbers shown in the formula
    • In a balanced chemical equation, the sum of Mr of reactants in quantities shown = sum of Mr of products in quantities shown
    • If a reaction appears to involve a change in mass
      Check if this is due to a reactant or a product as a gas and its mass has not been taken into account
    • When a metal reacts with oxygen, the mass of the metal oxide product is greater than the mass of the metal
    • Whenever a measurement is made there is always some uncertainty about the result obtained
    • Estimation of uncertainty
      Be prepared to make estimations of uncertainty when making chemical measurements
    • Mole
      The unit used to measure chemical amounts
    • The mass of one mole of a substance in grams is numerically equal to its relative formula mass
    • One mole of a substance contains the same number of the stated particles, atoms, molecules or ions as one mole of any other substance
    • Converting between moles and grams
      Mass = moles x RFM
    • The number of atoms, molecules or ions in a mole of a given substance is the Avogadro constant: 6.02 x 10^23 per mole
    • Balanced symbol equation
      Can be interpreted in terms of moles
    • The total moles of one element must be the same on both sides of the equation
    • Balancing numbers in a symbol equation
      1. Convert masses in grams to amounts in moles
      2. Convert numbers of moles to simple whole number ratios
    • Limiting reactant
      The reactant that is used up / not in excess (since it limits the amount of products)
    • If a limiting reactant is used, the amount of product produced is restricted to the amount of the excess reactant that reacts with the limiting one
    • Concentration of a solution
      Measured in mass per given volume of solution e.g. grams per dm^3 (g/dm^3)
    • Calculating mass of solute in a given volume of a known concentration
      Mass = concentration x volume
    • Smaller volume or larger mass of solute

      Gives a higher concentration
    • Larger volume or smaller mass of solute

      Gives a lower concentration
    • Percentage yield
      Amount of product produced / Maximum amount of product possible x 100
    • Reasons why calculated amount of product may not be obtained
      • Reaction may not go to completion because it is reversible
      • Some of the product may be lost when it is separated from the reaction mixture
      • Some of the reactants may react in ways different to the expected reaction
    • Yield
      Amount of product obtained
    • Calculating theoretical mass of a product
      1. Calculate mol. of reactant by using mol. = mass / molar mass
      2. Use balancing numbers to find mol. of product
      3. Calculate theoretical mass of a product by using mass = mol. x molar mass
    • Atom economy
      A measure of the amount of starting materials that end up as useful products
    • Atom economy is important for sustainable development and for economic reasons to use reactions with high atom economy
    • Possible reasons why a particular reaction pathway is chosen/not chosen
      • Atom economy
      • Yield
      • Rate
      • Equilibrium position
      • Usefulness of by-products
    • Concentration of a solution
      Measured in mol. per given volume of solution e.g. mol. per dm3 (mol./dm3)
    • Calculating concentration
      1. Mass of solute
      2. Volume of solution
      3. Moles = concentration x volume
    • Calculating moles from mass
      Mol. = mass / molar mass
    • Calculating concentration from known moles and volume
      1. Moles = concentration x volume
      2. Concentration = moles / volume
    • Calculating concentration of unknown solution
      1. Work out moles of known solution
      2. Use mole ratio from equation to find moles of unknown solution
      3. Concentration = moles / volume
    • If the volumes of two solutions that react completely are known and the concentration of one solution is known, the concentration of the other solution can be calculated
    • Equal amounts (in mol.) of gases
      Occupy the same volume under the same conditions of temperature and pressure (e.g. RTP)
    • Volume of 1 mol. of any gas at RTP (room temperature and pressure: 20 degrees C and 1 atmosphere pressure)

      24 dm3
    • Equation to calculate volume of gas at RTP
      Volume of gas (dm3) at RTP = Moles x 24
    • Using the equation, if the reaction is at RTP, you can calculate moles of a gas produced and then x24 to get volume produced (e.g. if you produce 5 moles of hydrogen, you produce 24 x 5 = 120 dm3)