Chapter 9
for the reaction represented by the equation 2H2+O2-->2H2O, how many grams of water are produced from 6.00 mol of hydrogen
108g
For the reaction represented by the equation 2H2+O2-->2H2O, how many moles of water can be produced from 6.0 mol of oxygen
12 mol
***For the reaction represented by the equation 2HNO3+Mg(OH)2-->Mg(NO3)2+2H2O, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO3
593g
For the reaction represented by the equation N2+3H2-->2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia
9.0 mol
***For the reaction represented by the equation SO3+H20-->H2SO4, calculate the percentage yield if 500.g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid
93.9%
***Which brand of chem. deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions
stoichiometry
***Which coefficients correctly balance the formula NH4NO2-->N2H2O
1,1,2
The Haber process for producing ammonia commercially is represented by the equation N2+3H2-->2NH3. To Completely convert 9.0 mol hydrogen gas ammonia gas, how many moles of nitrogen gas are required?
3.0 mol
The reaction represented by the equation N2+3H2-->2NH3, what is the mole ratio of hydrogen to ammonia
3:2
In the equation 2KClO3-->KCl+3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely
4.5 mol
***For the reaction represented by the equation 2Na+2H2O-->2NaOH+H2, how many grams of hydrogen are produced if 120.g of sodium and 80. g of water are available
4.5g
for the reaction represented by the equation CH4+2O2-->2H2O+CO2, calculate the percentage yield of carbon dioxide if 1000g of methane react with excess oxygen to produce 2300 g of carbon dioxide
83.88%
When the formula equation Fe3O4+Al-->Al2O3+Fe is correctly balanced the coefficient of Fe is number
9
Which reactant controls the amount of product formed in a chemical reaction
limiting reactant
A balanced chemical equation allows one to determine the
mole ratio of any two substances in the reaction
what is the mole ratio of the actual yield to the theoretical yield, multiplied by 100%
percentage yield
