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According to the following reaction, what mass of PbCl2 can form from 325 mL of 0.110 M KCl solution?  Assume that there is excess Pb(NO3)2. KCl = 74.548 g/mol; Pb(NO3)2  = 331.208 g/mol; PbCl2 = 278.1 g/mol; KNO3 = 101.102 g/mol             2 KCl(aq) + Pb(NO3)2(aq)  →  PbCl2(s) + 2 KNO3(aq)

Determine the percent yield of a reaction that produces 38.65 g of Fe when 60.00 g of Fe2O3 reacts with excess Al according to the following reaction.             Fe2O3(s) + 2 Al(s)  →  Al2O3(s) + 2 Fe(s)

A sample of potassium iodide is decomposed into its constituent elements.  If the sample produced 24.4 kg of potassium, how many kg of iodine were produced?

How many molecules of sucrose are contained in 14.3 mL of 0.120 M sucrose solution?

What element is undergoing oxidation (if any) in the following reaction? Zn(s) + 2 AgNO3(aq)  →  Zn(NO3)2(aq) + 2 Ag(s)

How many moles of nitrogen are formed when 78.6 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)

Determine the molarity of a solution formed by dissolving 59.8 g LiBr in enough water to yield 650.0 mL of solution.

How many moles of nitrogen are formed when 46.6 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 0.198 M KOH solution.  What is the concentration of the H3PO4 solution (in M)?

How many molecules of sucrose are contained in 14.3 mL of 0.120 M sucrose solution?