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Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed.

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution?  Hint:  You will want to write a balanced reaction.  AgNO3 = 169.874 g/mol; Na2SO4 =  142.036 g/mol

How many moles of nitrogen 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)

How many grams of Li3N can be formed from 0.95 moles of Li?  Assume an excess of nitrogen.             6 Li(s) + N2(g)  →  2 Li3N(s)

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)

How many moles of nitrogen are formed when 54.6 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)

A sample of potassium iodide is decomposed into its constituent elements.  If the sample produced 26.4 kg of potassium, how many kg of iodine were produced?

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 65.0 g N2O4 and 50.0 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 nitrogen 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)

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.138 M KOH solution.  What is the concentration of the H3PO4 solution (in M)?