202g HCL
20 moles
Molar Ratio
320g
Percent yield
8.32 moles HCL
3:2
574g FeO
6.022 * 10^23
True
% Yield= (Actual YIeld/Theoretical Yield) * 100
~40.0g
Limiting Reactant
22.4 L
What you actually make during the experiment
Conversion factor that relates the amount of moles of any two substances involved in a chemical reaction.
12 moles
relative numbers of moles of reactants and products
the reaction stops
Balance the Equation
The limiting reactant
Excess Reactant
the maximum amount of product that can be produced from a
4:3
114.16g/mol
(T/F) Throughout chapter nine we have been studying reaction stoichiometry?
For the reaction HCl + NaOH → NaCl + H2O, how many moles of hydrochloric acid are required to produce 150. g of water?
What is molar mass of C6H10O2
For the reaction 2H2 + O2→ 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?
What is the formula for Percent Yield?
For the reaction SO3 + H2O → H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid?
For the reaction 2Fe + O2 → 2FeO, how many grams of Oxygen are required to produce 350 g of FeO
What is the definition of Mole Ratio?
The ratio of the actual yield to the theoretical yield multiplied by 100
The substance that is not used up completely in a chemical reaction?
The coefficients in a chemical equation represent the
In the reaction 2Al2O3 → 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
For the reaction HCl + NaOH → NaCl + H2O, how many grams of hydrochloric acid are required to produce 100 g of water?
What is the actual yield?
What is the measurement for volume @ STP?
For the reaction 2Fe + O2 → 2FeO, how many grams of iron oxide are produced from 8.00 mol of iron?
Avagadro's Number is 1 mole = ?
In the reaction 2Al2O3 --> 4Al + 3O2, what is the mole ratio of Oxygen to Aluminum Oxide??
What is the first step to take before calculating a stoichiometry problem?
What is the definition of theoretical yield?
In the reaction A + B → C + D, if the quantity of B is insufficient t, then B is what?
When the limiting reactant in a chemical reaction is completely used, the reaction....?
A balanced chemical equation allows one to determine the
The reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction?
For the reaction C + 2H2 --> CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4?
