Stoichiometry Ch.10

(10-1) Stoichiometry Mass & amt relationships b/w reactants & products –Conversions b/w grams & moles Always begin w/ a balanced eq.!

Mass to Mol Reminder Convert 3.5 g of NaOH to mols NaOH 1.List known 3.5 g NaOH 2.Calculate molar mass g/mol Na + 16 g/mol O g/mol H = 40 g/mol 3.Set up problem & solve 3.5 g NaOH x 1 mol NaOH = 0.09 mol NaOH 40 g NaOH

Mol to Mass Reminder How many grams are in 6.4 mols O 2 ? 1.List known 6.4 mols O 2 2.Calculate molar mass (2) (16 g/mol O) = 32 g/mol O 2 3.Set up problem & solve 6.4 mols O 2 x 32 g O 2 = g O 2 1 mol O 2

Mol to Mol Reminder If 2.00 mol N 2 is reacting w/ a sufficient amt of H 2, how many mols of NH 3 will be produced? N 2 + H 2  NH 3 1.Balance the chemical eq. N 2 + 3H 2  2 NH 3

Mol to Mol Reminder 2.Find the mole ratio 1 mol N 2 : 2 mol NH 3 3.Set up problem (begin w/ known) & solve 2.00 mol N 2 x 2 mol NH 3 = 4 mol NH 3 1 mol N 2

Conversions g of A  mol of A  mol of B  g of B Mole ratio (coeff.from bal.eq.) Molar Mass (from PT) Molar Mass (from PT)

Mass to Mass Practice How many grams of H 2 O are produced when 13 g O 2 combine w/ sufficient H 2 ? H 2 + O 2  H 2 O 1.Balance the chemical eq. 2 H 2 + O 2  2 H 2 O

Mass to Mass Practice 2.Calculate molar mass of known & unknown O 2 = 32 g/mol H 2 O = g/mol 3.Find mole ratio 1 mol O 2 : 2 mol H 2 O

Mass to Mass Practice 4. Set up problem (begin w/ known) & solve 13 g O 2 x 1 mol O 2 x 2 mol H 2 O x g H 2 O 32 g O 2 1 mol O 2 1 mol H 2 O = g H 2 O

Using Density Density (D) = mass (m) / volume (V) Units: g/mL Convert from g  mL or mL  g

Density Practice Calculate the mass of LiOH used to obtain 1500 mL of water. (Hint: D H 2 O = 1.00 g/mL) CO 2 + 2LiOH  Li 2 CO 3 + H 2 O 1.Start w/ known & use density to convert into grams 1500 mL H 2 O x 1.00 g H 2 O 1 mL H 2 O

Density Practice 2.Proceed w/ mass to mass calc mL H 2 O x 1.00 g H 2 O x 1 mol H 2 O x 1 mL H 2 O g H 2 O 2 mol LiOH x g LiOH = 3989 g LiOH 1 mol H 2 O 1 mol LiOH

(10-2) Excess Reactant Extra left over after rxn Limiting reactant: completely consumed –Limits amt of other reactants used –Determines max amt of product

Limiting Reactant Practice CO combines w/ H 2 to produce CH 3 OH. If you had g CO & 24.5 g H 2 what mass of CH 3 OH could be produced? 1.Write a bal. eq. CO + 2 H 2  CH 3 OH

Limiting Reactant Practice 2.Convert reactants to mols present g CO x 1 mol CO = mol CO present g CO g H 2 x 1 mol H 2 = 12.1 mol H 2 present 2.02 g H 2

Limiting Reactant Practice 3.Using the reactants mol ratio, find how many mols needed 12.1 mol H 2 x 1 mol CO = 6.06 mol CO needed 2 mol H 2 CO present is not enough to react w/ all the H 2, so CO is limiting

Limiting Reactant Practice 4. Use limiting reactant to set up stoich mol CO x 1 mol CH 3 OH x g CH 3 OH 1 mol CO 1 mol CH 3 OH = g CH 3 OH

Theoretical Yield Calculated max amt of product possible –Stoich. w/ limiting reactant –What should happen Actual yield: measured amt of product experimentally produced –What does happen

Percentage Yield How efficient a rxn is –How close actual is to theoretical –Should be 100% % yield = actual x 100 theoretical

% Yield Practice When mol LiOH is reacted w/ excess KCl, the actual yield of LiCl is 16 g. What is the % yield? LiOH + KCl  LiCl + KOH

% Yield Practice 1. Calculate the theor. yield mol LiOH x 1 mol LiCl x g LiCl = 35.4 g LiCl 1 mol LiOH 1 mol LiCl 2.Calculate the % yield % yield = act. X 100 = 16 g LiCl x 100 = 45 % theor g LiCl