Terminology
The study of quantitative relationships between amounts of reactants and products in a chemical reaction.
What is Stoichiometry?
A mole ratio is obtained from __________.
The coefficients in a balanced chemical equation.
When a conversion factor includes grams and moles, what number goes with moles and what value goes with grams?
Grams: Molar Mass
What is the formula for percent yield?
actual
_____________ x 100
theoretical
Define Limiting Reactant.
A reactant that runs out first and is completely used up in a reaction.
States that mass of reactants must always equal the mass of the products.
What is the Law of Conservation of Mass?
A mole ratio is ______________. (there are multiple correct answers)
A fraction
A conversion factor
A ratio
Fe2O3 + 3 CO → 2 Fe + 3 CO2
65 grams of Fe2O3 are reacted with CO to form 45 grams of Fe and 54 grams of CO2. How many grams of CO reacted?
34 grams of CO
Calculate the percent yield given the following:
Theoretical: 155 g
Actual: 45 g
29%
Define Excess Reactant.
A reactant that is left over at the end of the reaction.
Numbers written in front of symbols or formulas in a chemical equation. They are used to balance the equation.
What is a coefficient?
What is the ratio of AlCl3 to AgCl in the following balanced equation?
AlCl3 + 3 AgNO3 → 3 AgCl + Al(NO3)3
1 mol AlCl3 : 3 mol AgCl
2H2 + O2 → 2H2O
How many moles of oxygen are needed to react with 6.0 moles of H2?
3 mol O2
Percent yield should always be ______ than 100%.
Less than 100%
Which type of reactant determines how much product can be made?
The limiting reactant.
In order to complete a stoichiometry problem, you must have a _______________.
Balanced Chemical Equation
How many mole ratios can you write from the following equation?
N2 + 3 H2 → 2 NH3
6
N2 + 3H2 → 2NH3
How many grams of NH3 will be produced from 5.7 moles of H2?
MOLAR MASSES
NH3 - 17.04 g/mol
H2 - 2.02 g/mol
65g NH3
What is actual yield and how do you determine it?
How much product is actual obtained when completing the reaction experimentally.
It must be provided in the problem.
A candle is burning in the room. You put the lid on the candle and the fire goes out. What is the limiting reactant?
Oxygen
Coefficients in a chemical equation represent _______________. (there are 2 correct answers)
Number of moles
OR
Number of particles
Balance the following equation AND name a possible mole ratio.
KClO3 → KCl + O2
2 KClO3 → 2 KCl + 3 O2
2Na + Cl2 → 2NaCl
How many grams of NaCl will be produced from 65.8 grams of Cl2?
MOLAR MASSES
NaCl - 58.44 g/mol
Cl2 - 70.90 g/mol
108g NaCl
It is the maximum amount of product that can be obtained.
It is found completing a mass to mass stoichiometry conversion (unless given in the problem).
2H2 + O2 → 2H2O
You have 6 moles of H2 and 4 moles of O2. Which reactant are you going to run out of first?
Hydrogen (H2)