Consider the reaction.
Mn3N2 (s) +H2O (l) → Mg(OH)2 (s) + NH3 (g)
a) Balance the equation and name each compound.
b) How many moles of Mg(OH)2 are produced from .319 mol of magnesium nitride?
c) How many grams of water are necessary to produce 4.39 mol of ammonia?
d) If 12.48g of magnesium hydroxide are formed, how many grams of ammonia are produced?
-Start with 2.95g of magnesium nitride and 1.500g of water.
a) What is the limiting reactant?
b) How many grams of magnesium hydroxide can be theoretically obtained?
c) If only 2.009g of magnesium hydroxide are obtained, what is the percent yield of the reaction?
Solution answers 2 questions with multiple parts including concepts like equation-balancing, moles produced, water necessary, limiting reactants and percentage yield for reactions. Attached as Word.