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Chapter 3Stoichiometry
Deals with quantities of materials consumed and produced in chemical reactions
Stoichiometry Terms Atomic Mass
-Average value of the isotopes in a naturally occurring element-Sometimes called the atomic weight
Mole- the number equal to the number of carbon atoms in exactly 12 grams of pure Carbon-12- symbol is mol
Terms con. Avogadro’s Number
- one mole of anything contains 6.022 x 1023 units of that substance
- Mass of 1 mol of an element= its atomic mass in grams
- One mole of Al= 6.022 x 1023 atoms of Al
Examples Determine the number of moles of atoms
and the number of atoms I a 10.0 g sample of aluminum.
Calculate the number of moles in a sample of cobalt containing 5.00 x 1020 atoms and calculate the mass of the sample.
Molar Mass Mass in grams of 1 mole of the compound Example: Calcium carbonate(CaCO3) is
found in limestone, marble, and chalk. Determine its molar mass. If a sample contains 4.86 moles, determine its mass and the mass of carbonate ions present?
Another example Calculate the number of molecules in 1.058
moles of H20.
Percent Compostion of Compounds
Percent by mass of each element present in a compound1. Determine the molar mass of the compound2. Divide the mass of each element by the total molar mass
Example: Determine the mass percent of each element in glucose, C6H12O6.
Determining the Formula of a Compound
Two Types of Formulas
1. Emperical formula
- the simplest whole number ration of atoms in a compound
2. Molecular Formula
- exact formula of a compound
- molar mass of the compound is needed
Examples of Emperical and Molecular
Emperical Molecular
H2O H2O
CH2O C6H12O6
Determining the Emperical formula
You need to convert % composition to empirical formula
Percent to mass Mass to moles Divide by small Multiply ‘til whole
Example of Emperical Formula A compound consists of the following:
71.65 % Cl 24.27% C 4.07% H
Determine its emperical formula.
Determining the Molecular Formula
1. Determine the emperical formula
2. Calculate the emperical formula mass
3. Divide the molar mass of the compound by the emperical formula mass
4. Multiply the emperical formula subscripts by this factor
Molecular formula example From a previous example, the empirical
formula was ClCH2. The molar mass of the compound is 98.96 g/mol. What is the molecular formula?
Chemical Equations Represents a chemical reaction showing the #’s of
reactants and products Types of Info found in an Equation
1. Nature of the reactants/products Solid(s) Liquid(l) Gas(g) Dissolved in water(in aqueous solution)(aq)
2. Relative # of each reactant and product
Balancing Chemical Equations CH4 + O2 CO2 + H20
Coefficient- used to balance equations 1. Tells how many moles of
reactants/products 2. Tells how many molecules involved in the
reaction
Balancing examples Solid ammonium dichromate when ignited
produces solid chromium(III) oxide, nitrogen gas, and water vapor. Write a balance equation.
Ammonia gas, NH3, reacts with oxygen gas to form gaseous nitric oxide, NO, and water vapor. Write a balanced equation.
Stoichiometric Calculations What mass of oxygen will react with 96.1 g
of propane, C3H8, to produce carbon dioxide and water vapor?
5 O2(g) + C3H8(g) 3 CO2(g)+ 4 H2O(g)
Calculations involving a Limiting Agent
Limiting Reactant Reactant that is consumed first and limits the number
of products
Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high temperatures. The other products are solid copper and water vapor. If a sample containg 18.1 g of NH3 is reacted with 90.4 g of CuO, which is the limiting agent? How many grams of N2 will be formed?
Calculating Percent Yield Theoretical Yield- amount of a product
formed when a limiting reactant is completely consumed
% yield= actual yield/theoretical yield • 100
Percent yield example Methanol(CH3OH) can be manufactured by
a combination of gaseous carbon monoxide and hydrogen. Suppose 68.5 kg CO(g) is reacted with 8.60 kg H2(g). Calculate the theoretical yield of methanol. If 3.57 x 104 g of methanol is actually produced, what is the % yield of methanol?