1. Is this a balanced eq ? 332

2. 332

6. We only need ONE information during the reaction (reacted or produced)

7. Another Example

8. Ratio in the stoichiometric equation : 3/1 = 3.00 Ratio in the feed : 21/15 = 1.40 C to Fe 2 O 3 in the feed is < that in the equation Therefore C is the LR

11. 15 moles Fe 2 O 3 - 21 mol C x 1 mol Fe 2 O 3 3 21 mol C x 1 mol Fe 2 O 3 3 % Excess Fe 2 O 3 = ( Note : In the calculation of %excess ER, we assume the rxn is complete even if is actually not complete ) moles ER in – Moles ER reacting with all LR in Moles ER reacting with all LR in =

12. % Completion of a reaction = moles ( or mass ) of a reactant A consumed x 100 moles ( or mass ) of a reactant A fed (entering) NOTE: Normally the reactant we use for this calculation is the limiting reactant moles (or mass) of a product formed moles (or mass) of a reactant fed Yield =