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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)?

Determine the molarity of a solution formed by dissolving 89.7 g LiBr in enough water to yield 750.0 mL of solution.

According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted?  A few of the molar masses are as follows:  Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol.               Al2S3(s) + 6 H2O(l)  →  2 Al(OH)3(s) + 3 H2S(g)

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?

How many moles of oxygen are formed when 38.6 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 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)

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)

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?

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)