Mass to Mass EXAMPLES:
Lead (IV) nitrate reactions with 5.0 g of Potassium iodide.
Grams of Lead (IV) Nitrate are required?
Pb(NO3) + 4 KI -----> 4 KO3 + PbI45.0 g x 1 mol KI/165.9 g x 1 Pb(NO3)4/4KI x 455.2/ 1 mol Pb(NO3)4 = 3.4 gif a 100 mL solution of 2.0 M H2SO4 is neutralized by sodium hydroxide what mass of water is produced?
H2(SO4) + NaOH -----> HOH + Na2(SO4)2.0 mol/L x .1 L = .200 mol H2(SO4) x 2 HOH/1 H2(SO4) x 18.0 g/mol = 7.2 g H2OPercent Yield
The theoretical yield of the reaction is the expected *calculated* amount. The experimental amount is the actual yield% yield = actual/theoretical x 100
IE: He production of urea CO(NH2) is given by:
2NH3 + Co2 -----> CO(NH2) + H2O. 47.7 g of urea are produced when 1 mole of CO2 reacts, find the actual yield, theoretical yield and percent yield.
The actual yield is 46.7 g.
The theoretical yield: 1 mol CO2 x 1 CO(NH2)2/1 CO2 x 60.1 g/ 1 mol = 60.1 g
Percent Yield = 47.7 g/60.1 g x 100 = 79.4%
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