Mole Ratios in Chemical Equations LG: I can predict the amount (moles) of reactant or product used or created during a chemical reaction

Mole Ratios Balanced chemical equations indicate the ratio of one chemical to another used in a reaction This ratio indicates the relative number of entities, not the mass, of each substance Example: 2 H2(g) + O2(g)  2 H2O(g) 2 molecules of hydrogen reacts with 1 molecule of oxygen to produce 2 molecules of water OR 2 moles of hydrogen react with every one mole of oxygen to produce two moles of water. Mass is conserved from reactants  products, but the number of entities is not; 3 moles of reactants produce 2 moles of product.

Gimme S’more Stoichiometry! Use the recipe for S’mores to investigate the ratios of reactants and products in chemical reactions

Example The Haber process is used to manufacture ammonia, used in fertilizer, from hydrogen and nitrogen gas N2(g) + H2(g)  NH3 Balance the equation above to determine the mole ratio in the reaction How many moles of hydrogen would be required to react with 6.2 mol of nitrogen gas? If the amount of nitrogen was unlimited, how many moles of ammonia could be produced from 10.8 mol of hydrogen? If you had 3.0mol of N2 and 8.0mol of H2, which substance would run out first (limiting reagent)? How much product could be made? How much excess reagent would remain after the reaction? German chemist, Fritz Haber discovered process in 1913. Used in WWI to make explosives..prolonged war and cost many lives, but also increased crop yields and most likely prevented many deaths from starvation

Homework Complete Mole Ratios Handout