Q1: 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)
Q2: Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
Q3: Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 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)
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