Moles. Stoichiometry The study of quantitative relationships between the amounts of reactants used...
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Transcript of Moles. Stoichiometry The study of quantitative relationships between the amounts of reactants used...
Moles
Stoichiometry
The study of quantitative relationships between the
amounts of reactants used and products formed by a chemical
reactions; it is based on the law of conservation of mass.
MoleThe SI base unit used to measure the amount of a
substance.
Avogadro’s NumberThe number of representative particles in a mole, and can be
rounded to three significant digits: 6.02 X 1023
molecules/mol (atoms/mol)(formula units/mol)
(electrons/mol)
Molecule Forms when two or
more atoms covalently bond.
A number smaller than 1.0 x 1019 or greater
than 1.0 x 1026 should not be found in front of molecule or atom.
To find the number of molecules it takes to equal a certain number of moles. Take the number of moles
given and multiply by Avogadro’s number.
How many molecules of Sucrose is in 3.50 moles of
Sucrose.
3.50 mol Sucrose X 6.02x1023 molecules/mol =2.11x1024molecules of Sucrose
How many molecules of Sodium Hydroxide is in 4.80 moles of Sodium Hydroxide?
4.80 mol Sodium Hydroxide X
6.02x1023molecules/mol
=2.89x1024 molecules of Sodium Hydroxide
To find the number of moles it takes to equal a
certain number of molecules. Take the
number of molecules given and divide by Avogadro’s
number.
How many moles of Sucrose is in 3.54x1024 molecules of Sucrose.
3.54x1024 molecules of Sucrose ÷
6.02x1023 molecules/mol
=5.88 moles of Sucrose
How many moles of Sodium Hydroxide is in 5.63x1024
molecules of Sodium Hydroxide.
5.63x1024 molecules NaOH ÷6.02x1023 molecules/mol=9.35 moles of NaOH
A number smaller than 0.0001 or greater than
10,000 should not be found in front of grams.
Atomic MassThe weighted average mass of the isotopes
of that element.
Mass Number
The number of protons plus the number of
neutrons found in that element
Molar MassThe mass in grams of one mole of any pure
substance.
g/mol
To find the number of grams of substance. Take the number of moles given
and multiply by the substance’s molar mass.
Find the mass of 3.2 moles of Butane needed to
complete the reaction.
3.2 mol of Butane X
58.14 g/mol
=186.05 g of Butane
Find the mass of 4.5 moles of Pentanol needed to complete the reaction.
4.5 mol Pentanol X86.15 g/mol=387.68 g of Pentanol
To find the number of moles of substance. Take the number of grams given
and divide by the substance’s molar mass.
Find the moles of 23 g of water needed to complete
the reaction.
23 g water ÷18.02 g/mol=1.28 mol of water
Find the moles of 112 g of Hydrochloric Acid needed to complete the reaction.
112 g of Hydrochloric Acid ÷36.46 g/mol=3.07 mol of Hydrochloric Acid
To find the number of moles of an element in a compound, multiply the moles of the compound
with the ratio of number of elements to 1 mol of
compound.
How many moles of Fluorine is found in 5.50 moles of
Freon (CCl2F2).
5.50 mol CCl2F2 X
2 mol F atoms/1 mol CCl2F2 = 11.0 mol F atoms
How many moles of Oxygen is found in 4.75 moles of
Glucose (C6H12O6).
4.75 mol C6H12O6 X 6 mol O atoms/1 mol C6H12O6 = 28.5 mol O atoms
Molecular MassThe mass of the
molecule found by adding the mass of each atom in the
molecule.
To find the molar mass of compound, for each element multiply the
number of element with the ratio of the molar mass of the element to 1 mol of the element. Add all the grams
up.
What is the molar mass of Potassium Chromate K2CrO4.2molK X 39.1gK/1molK=78.2g
1molCr X 52gCr/1molCr=52g
4molO X 16gO/1mol=64g
78.2g + 52g + 64g=194.2g K2CrO4
What is the molar mass of Sodium Hydroxide NaOH.
1molNaX22.99gNa/1molNa
=22.9g
1molH X 1.01gH/1molH=1.01g
1molO X 16gO/1mol=16g
22.9g+1.01g+16g=39.9gNaOH
To find the moles of a compound, take the mass
of the compound and divide by the molar mass of
the compound.
How many moles are there of 47g of water?
47g of water ÷
18.02 g/mol of water
= 2.61 mol of water
How many moles are there of 21g of Benzene?
21g of Benzene ÷
78.12 g/mol of Benzene
= 0.27 mol of Benzene