Stoichoimetry
For the equation P4(s) + 5O2(g) -> P4O10(s), if 3 mol of phosphorus react with 10 mol of oxygen, the theoretical yield of phosphorus(V) oxide will be
2 mol
Ozone, O3, is produced in automobile exhaust by the reaction represented by the equation NO2(g) + O2(g) -> NO(g) + O3(g). What mass of ozone is predicted to form from the reaction of 2.0 g NO2 in a car's exhaust and excess oxygen?
2.1g O3
If the percentage yield for the reaction represented by the following equation is calculated to be 75.3%, what mass of Al is expected from the reaction of 52.5 g of Al2O3? 2Al2O3(l) -> 4Al(s) + 3O2(g)
20.9 g Al
What is the mole ratio of H2O to H3PO4 in the following chemical equation? P4O10 + 6H2O -> 4H3PO4
3:2
In the equation 2Al2O3 -> 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
4:3
2Fe + O2 → 2FeO; how many grams of iron oxide will be produced from 8.00 mol of iron when O2 is in excess?
575 g FeO
For the reaction represented by the equation N2 + 3H2 -> 2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia?
9
For the reaction represented by the equation SO3 + H2O -> H2SO4, what is the percentage yield if 500. g of sulfur trioxide reacts with excess water to produce 575 g of sulfuric acid?
93.9%
The measured amount of product obtained from a chemical reaction is called the
Actual yield
If, in the reaction A + B → C + D, the quantity of B is insufficient to react with all of A:
B is the limiting reactant
The substance that is not completely used up in a chemical reaction is known as the
Excess reactant
The substance that restricts the amount of other reactants used in a chemical reaction is known as the
Limiting reactant
In the formation of silicon carbide represented by the chemical equation SiO2(s) + 3C(s) -> SiC(s) + 2CO(g), 8 mol of each reactant are available for the reaction. What substance is the excess reactant?
SiO2(s)
The measured amount of product obtained from a chemical reaction is the
actual yield
If the percentage yield for a chemical reaction is 80.0%, the
actual yield is 80.0g for every theoretical yield of 100.g
When a chemical reaction is carried out under ideal conditions, it is implied that
all reactants are completely converted into products
The chemical equation P4O10 + 6H2O -> 4H3PO4 can be interpreted correctly as
both (a) and (b)
The actual yield of a chemical reaction is generally
less than the theoretical yield
The participation of reactants in a chemical reaction is restricted by the
limiting reactant
A balanced chemical equation allows one to determine the
mole ratio of any two substances in the reaction
The efficiency of a chemical reaction is best expressed by the
percentage yield
Reaction stoichiometry is based on chemical equations and
the law of conservation of mass
The number of significant figures in an answer to a stoichiometry problem is determined by
the number of significant figures of any measured quantities in the problem
Molar masses are determined from
the periodic table
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
theoretical yield
The limiting reactant of a reaction can be used to calculate the
theoretical yield
For the reaction represented by the equation Pb(NO3)2 + 2KI -> PbI2 + 2KNO3, how many moles of lead iodide are produced from 300. g of potassium iodide when Pb(NO3)2 is in excess?
0.904 mol PbI2
If cyclohexanol is burned as a fuel according to the following equation, how many moles of oxygen are needed to produce 13.7 mol of carbon dioxide? 2C6H12O + 17O2 -> 12CO2 + 12H2O
19.4 mol O2
In the chemical reaction: 4Fe(s) + 3O2(g) -> 2Fe2O3(s), the mole ratio of iron (III) oxide to iron is
1:2