Answer:
When no coefficient is written in front of a formula it is assumed to be 1. 4. Numbers appearing in the formulas are known as subscripts. These can never be changed when balancing the equation or you will change the identity of the substance.
Explanation:
1. Reactants go on the left hand side and products go on the right hand side of a chemical equation. Be sure to write the correct formulas for the reactants and products.
· Remember atoms are conserved in a chemical reaction. ie they are neither created or destroyed. So all the atoms in the reactants must end up somewhere among the products.
2. Count the number of atoms of each element, compound or ion in the reactants and products. If they are not equal proceed further.
3. Balance the atoms one at a time by placing coefficients in front of the formula so that the numbers of atoms of each element are equal on both sides of the equation. Remember atoms may exist in an element, compound or ion.
· It is usually easier to start with the atoms that occur in only one substance on each side of the equation.
· Balance the atoms that occur in compounds before attempting to balance atoms that occur in elemental form. e.g. H2, O2 or Cl2
· To make it easier if a polyatomic ion appears unchanged on both sides of the equation treat it as a whole unit.
· When no coefficient is written in front of a formula it is assumed to be 1.
4. Numbers appearing in the formulas are known as subscripts. These can never be changed when balancing the equation or you will change the identity of the substance.
· Remember with subscripts, any number to the right of parentheses multiplies each subscript within the parentheses.
eg Fe2(SO4)3 contains 2 Fe atoms, 3 S atoms and 12 O atoms.
5. Finally make sure that all the coefficients are in the smallest possible whole number ratio.
