Mole to Mass and Other Conversions

Examples
1. Lead(II) Nitrate reacts with 5.0g of potassium iodide. How many grams of Lead(IV) nitrate are required for a complete reaction?

Step 1. Find balanced equation
Pb(NO3)4 + 4 KI-> PbI4 + 4 KNO3

Step 2. Convert and multiply what you need over what you're given
5.0g x 1mol/166g x 1Pb(NO3)4/4KI x 455.2g/1mol Pb(NO3)4 = 3.5g


2. How many grams of O2 are produced from the decomposition of 3.0g of potassium chlorate?

Step 1. Find balanced equation
2 KClO3 -> 2 KCl + 3 O2

Step 2. Convert and multiply what you need over what you're given
3.0g x 1mol/122.6g x 3mol of O2/2mol of KClO3 x 32g/1mol of O2 = 1.2g


3. If a 100mL solution of 2.0M H2SO4 is neutralized by sodium hydroxide. What mass water is produced?

Step 1. Find balanced equation
H2SO4 + 2 NaOH -> 2 HOH + Na2SO4

Step 2. Convert(in this case use concentration formula to find the number of mol) and multiply what you need over what you're given
0.100L x 2.0mol/1L = 0.200mol H2SO4 x 2mol HOH/1mol H2SO4 x 18.0g/1mol = 7.2g

*Remember for next class' lab*
-Theoretical yield of a reaction is the quantity of products expected(calculation)
-The amount produced in an experiment is the actual yield
-The percent yield is : %yield = actual/theoretical x 100