things you must know and what to expect things you must know you must know your polyatomics you...
TRANSCRIPT
Things you must KNOW and what to expect Things you must KNOW
You must KNOW your polyatomics
You must KNOW how to write a balanced formula
You have to be able to balance a chemical equation
You need to know how to convert from grams to moles and moles to grams.
You need to be able to calculate molar mass
What to expect in this chapter You will be converting grams to moles of one
compound, then using the mole ratio (balanced equation) go to moles of another compound and then from moles to grams in the new compound.
You will learn how to identify a limiting reactant, and how to calculate percent yield.
What is Stoichiometry?
Stoichiometry: the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction.
Based on the Law of Conservation of Mass
(mass reactants = mass products)
To prove Law of Conservation of Mass
1. Start with a balanced equation
2. Coefficient indicates the #molecules/formula units and # of moles
3. Change moles to mass
4. Add up mass reactants and mass of products
They should equal
C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g)
What is Stoichiometry? : continued
Can use balanced chemical equation to get mole ratios
2 Al + 3 Br2 2 AlBr3
2 mol Al 2 mol Al 3 mol Br2
3 mol Br2 2 mol AlBr3 2 mol AlBr3
Find all the possible mole ratios for:
KClO3(s) KCl(s) + O2(g)
Stoichiometric Calculations
Use relationships to determine the amount of product formed or reactant needed. Moles to moles
Moles known x mol unknown
mol known
from problem
ratio from balanced
equation
=mol unknown
Moles MolesHow many moles of carbon
dioxide are produced when 10.0 moles propane (C3H8) are burned in excess oxygen?
1. Write & balance the equationC3H8 + 5 O2 3 CO2 + 4 H2O
2. Find the mole ratio between propane and carbon dioxide: 1 mol C3H8 : 3 mol CO2
3. Multiply ratio by known amount from problem
10 mol C3H8 x 3 mol CO2 = 30 mol O2
1 mol C3H8
Moles Mass
Moles to massDetermine the mass of sodium needed when sodium reacts with 1.25 moles of chlorine gas to form sodium chloride
1. Write & balance the equation2 Na + Cl2 2 NaCl
2. Find the mole ratio between propane and carbon dioxide: 2 mol Na: 1 mol Cl2
3. Multiply ratio by known amount from problem
1.25 mol Cl2 x 2 mol Na = 2.50 mol Na 1 mol Cl2
4. Change moles to grams
2.50 mol Na x 22.99 g Na = 57.48 g Na 1 mol Na
Mass Mass
Mass to mass
25.0 g NH4NO3 produces N2O and H2O when it decomposes. Find the mass of water produced.
1. Start with a balanced equationNH4NO3 N2O + 2 H2O
2. Change grams to moles25.0g NH4NO3 x 1 mol NH4NO3 = 0.312 mol NH4NO3
80.04g NH4NO3
3. Find the mole ratio : 1 mol NH4NO3 : 2 mol H2O
4. Multiply ratio by known amount from problem
0.312 mol NH4NO3 x 2 mol H2O = 0.624 mol H2O
1 mol NH4NO3
5. Change moles to grams
0.624 mol H2O x 18.02g H2O = 11.2 g H2O 1 mol H2O
Limiting Reactants
Limiting reactant: the reactant that runs out first
Excess reactant: the reactant that is left over
To solve limiting reactant problems:
1. Work the problem using both reactants and solve the number of moles produced of the same product The one that produces the least amount of moles is the
limiting reactant
Percent Yield
Theoretical yield is the maximum amount of product that can be produced (determined through stoichiometric calculations)
Actual yield is the amount produced in lab/from experiment Percent yield is the ratio of actual to theoretical expressed
as a percent.% yield = actual yield x 100
theoretical yield
Reasons for a decrease in percent yield Loss of products or reactants (spill, stick to side of containers) Human error Not all reactants react
Percent Yield continued
CH4 + 2 O2 CO2 + 2 H2O
Determine the % yield if 10.0 grams methane burned to produce 19.5 g water.
1. Use stoichiometric calculations to determine theoretical yield of water produced from 10.0 g methane.
2. Using 19.5 g H2O as the actual yield, solve for % yield.