Presentation on theme: "Balancing Chemical Equations"— Presentation transcript:
1 Balancing Chemical Equations Year 10 Physical ScienceFundamentals of Chemistry
2 Chemical ReactionsA Chemical Reaction is a process by which a substance is changed into one or more different substancesIndications of a chemical reaction include:Heat and lightProduction of gasFormation of a precipitateColor change
3 Chemical EquationsA chemical equation is a symbolic way of representing a chemical reaction.It shows the formulae all reactants and products and their physical states.The equation may also indicate conditions necessary for the reaction to occur.The states of the reactants and products should be indicated in the equation by:(s) for solid(l) for liquid,(g) for gas and(aq) for a solution of water
4 Chemical EquationsWhen writing chemical equations, you need to consider:Law of Conservation of Mass“In a chemical reaction, the total mass of the products equals the total mass of the reactants”Law of Constant Proportions“The same compound, however formed, contains the same elements chemically combined, in constant proportions by weight”
5 Balancing Chemical Equations The total mass of the reactants in a chemical reaction is equal to the total mass of the products.Atoms are not created or destroyed, but are rearranged to form new substances.A balanced chemical equation has the same number of each type of atom on each side of the equation.Balancing is achieved by placing numbers (coefficients) in front of each formula.We cannot change the formula of any substance in the equation, as these are found by experiment.
6 Rules for Balancing Chemical Equations 1. Write the reactants and products using the correct formula and state for each substance.Count the number of atoms of each element on the LHS of the equation.Do the same for the RHS and compare for each element.If any of these numbers don’t match, the equation is not balanced and you’ll need to complete the following steps:
7 Rules for Balancing Chemical Equations 3. Balance by placing coefficients in front of the formulae.DO NOT CHANGE THE ACTUAL FORMULAIf any substance is present as an element, leave the balancing of it to last.4. Check all atoms or ions to ensure that they are balanced.5. Make sure that the coefficients are in their lowest possible ratio.
8 Combustion ReactionsWhen hydrocarbons burn in a plentiful supply of oxygen, they produce carbon dioxide and water.When a limited air supply is available, carbon monoxide may be formed in preference to carbon dioxide.When octane, C8H18, is burnt in air:2C8H18 (g) O2 (g) 16CO2 (g) H2O (g)When octane, C8H18, is burnt in an engine:2C8H18 (g) O2 (g) 16CO (g) H2O (g)
9 Acid-Base & Neutralisation Reactions When an acid reacts with a base to form a salt and water, a neutralisation reaction occurs:Acid + Base Salt + WaterHydrochloric acid reacts with the base sodium hydroxide to form sodium chloride and water:HCl (aq) + NaOH (ag) NaCl (aq) + H2O (l)
10 Acid-Base & Neutralisation Reactions Other common acid-base reactions are:1. Acid + Metal Salt + Hydrogen2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g)Acid + Metal Carbonate Salt + Carbon Dioxide + Water2HCl (aq) + Na2CO3 (aq) 2NaCl (aq) + CO2 (g) + H2O (l)3. Acid + Metal Oxide Salt + Water2HCl (aq) + CuO (s) CuCl2 (aq) + H2O (l)Acid + Metal hydroxide Salt + WaterH2SO4 (aq) + 2NaOH (aq) Na2SO4 (aq) + H2O
11 Precipitation Reactions Precipitation occurs when ions in solution “swap partners” to form a new compound of low solubility in water.This low-solubility compound forms as solid particles that eventually settle.It is called a precipitate.To predict whether a precipitate will form, you need to know which substances are soluble in water and which are insoluble.Solutions of sodium chloride and silver nitrate react to form a precipitate of silver chloride.NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3 (aq)
14 Ionic EquationsAn ionic equation shows the association of the ions that form the precipitate.The other ions that are present but remain in solution are termed spectator ions.Spectator ions are not shown in the ionic equation.
15 Ionic Equations - Rules Write the balanced chemical equation.Decide which substances are soluble and which will form precipitates.Expand the chemical equation by dissociating all the soluble compounds into their free ions.Cancel all free ions that are unchanged on both sides of the equation (the spectators).Write the net ionic equation.
16 Ionic Equations - Example Write a balanced ionic equation for the reaction between barium chloride and sodium sulphate:BaCl2 + Na2SO4 → BaSO NaClBaSO4 is insoluble and forms the precipitate.NaCl is soluble and forms the spectator ion.3. Ba2+ (aq) + 2Cl- (aq) + 2Na+ (aq) + SO42- (aq) →BaSO4 (s) + 2Na+ (aq) + 2Cl- (aq)Hence we get:Ba2+ (aq) + SO42- (aq) → BaSO4 (s)