How many grams of Li3N can be formed from 1.15 moles of Li?  Assume an excess of nitrogen.             6 Li(s) + N2(g)  →  2 Li3N(s)

A sample of potassium iodide is decomposed into its constituent elements.  If the sample produced 10.4 kg of potassium, how many kg of iodine were produced?

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 reacts with excess Al according to the following reaction.             Fe2O3(s) + 2 Al(s)  →  Al2O3(s) + 2 Fe(s)

How many moles of oxygen are formed when 36.8 g of KNO3 decomposes according to the following reaction?  The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s)  →  2 K2O(s) + 2 N2(g) + 5 O2(g)

A sample of potassium iodide is decomposed into its constituent elements.  If the sample produced 16.4 kg of potassium, how many kg of iodine were produced?

How many of the following compounds are soluble in water?  Fe(OH)2          LiNO3            NH4I   Li2S

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 40.0 g N2O4 and 35.0 g N2H4.  Some possibly useful molar masses are as follows:  N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.             N2O4(l) + 2 N2H4(l)  →  3 N2(g) + 4 H2O(g)

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction?  The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s)  →  2 K2O(s) + 2 N2(g) + 5 O2(g)

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.174 M Na2SO4 solution?  Hint:  You will want to write a balanced reaction.  AgNO3 = 169.874 g/mol; Na2SO4 =  142.036 g/mol

Purchase Discounts Lost is a financial expense and is reported in the “other expenses and losses” section of the income statement.