4. If 100.0g of nitrogen gas (N2) is reacted with 100.0g of hydrogen gas (H2) to form NH3. What are the limiting and excess reactants? Hint: Convert grams to moles for each reactant and then convert to moles of NH3. You need your balanced equation from answer 1 to determine the mole relationship between each reactant and the product NH3. Use the periodic table to determine the molar mass of all chemical formulas. Fill in the “?” blanks below to show your work.

Balanced equation: 1N2 (g) + 3H2(g)  2NH3(g)

Molar mass of H2 = g/mol

100.0"g " "H" _2×(1"mol " "H" _2)/( ? "g " "H" _2 )×(" ? mol N" "H" _3)/(" ? mol " "H" _2 )= ? "mol N" "H" _3

Molar Mass of N2 = g/mol

100.0"g " "N" _2×(1"mol " "N" _2)/(" ? g " "N" _2 )×(" ? mole N" "H" _3)/(" ? mol " "N" _2 )= ? "mol N" "H" _3

A. What is the excess reactant? Hint: it is the reactant above that makes the most amount of product

B. What is the limiting reactant? Hint: it is the reactant above that makes the least amount of product

C. What is the theoretical yield of ammonia of the reaction?
Molar mass of NH3 = g/mol

100.0"g " "N" _2×(1"mol " "N" _2)/( ? "g " "N" _2 )×( ? "mol N" "H" _3)/( ? "mol " "N" _2 )×(" ? g N" "H" _3)/( 1 "mol N" "H" _3 )= ? "g N" "H" _3