Unit 3: Chemical Equations and Stoichiometry Balancing Equations

Balancing Equations Remember the law of conservation of mass? When a chemical reaction occurs, no atoms are created or just destroyed – they are just rearranged amount of each element on the left side (reactants) must equal the amount of the same element on the right side (products)

Balancing Equations – The Steps! Write the unbalanced equation Ionic compounds – charges must add to zero Covalent compounds – use prefixes HOFBrINCl elements are diatomic when alone Example: hydrogen gas is written H2 Add phase if information given (write as subscript) Solid = (s) Gas = (g) Liquid = (l) Aqueous (dissolved in water or solution) = (aq)

Balancing Equations Example #1 Write the following chemical equation: Propane (C3H8) gas + Oxygen gas  Carbon dioxide gas + water vapor

Balancing Equations – The Steps! Put coefficients in front of each substance to get the quantities on the left side = the right side Use the smallest whole number coefficients possible.

Balancing Equations - Hints Save “singletons” for last (elements that are not bonded with other elements) Save oxygen for last (if there are no singletons) Save hydrogen for 2nd to last

Balancing Equations Example #1 Now let’s balance this equation… __C3H8(g) + __O2(g)  __CO2(g) + __H2O(g)

Balancing Equations Practice #1 Write and balance the following chemical equation: Lead (IV) sulfide solid + oxygen gas  lead (IV) oxide solid + sulfur dioxide gas

Balancing Equations Practice #2 Write and balance the following chemical equation: ammonium phosphate soln. + magnesium nitrate soln.  ammonium nitrate soln. + magnesium phosphate solid