chemical quantities
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Chemical Quantities. Calculate the mass of compounds. Calculate the volume of a given mass of a gas from its density at a given temperature and pressure. Calculate the molar volumes of gases from their densities at a given temperature and pressure and compare the calculated volumes. - PowerPoint PPT PresentationTRANSCRIPT
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Chemical Quantities
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· Calculate the mass of compounds.
· Calculate the volume of a given mass of a gas from its density at a given temperature and pressure.
· Calculate the molar volumes of gases from their densities at a given temperature and pressure and compare the calculated volumes.
· Solve problems requiring conversions between mass, and number of particles, and moles.
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We call this - Avogadro's Number
In one mole there is 6.02 x 1023 particles.
One mole contains 6.02 x 1023 of anything
6.02 x 1023 pencils is 1 mole of pencils6.02 x 1023 carbon atoms is 1 mole…6.02 x 1023 water molecules is 1 mole…
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The molecular mass of water is 18.0 µ ...
One mole of any particle has a mass equal to its total atomic/formula/molecular mass – IN GRAMS (g).
One mole of aluminum atoms has a mass of 27.0 g.
So...the molar mass of water is 18.0 g/mol.
The mass of one mole is called the molar mass - units are grams per mole (g/mol)
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Molar mass of lead (II) chloride, PbCl2 ?
1 particle of PbCl2 - 1 atom of Pb, 2 atoms of Cl
1 mole of PbCl2 - 1 mole of Pb, 2 moles of Cl
PbCl2 = 207.2 g/mol + 2(35.5 g/mol)= 278.2 g/mol
The molar mass of lead (II) chloride is 278.2 g/mol.
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What is the molar mass of ammonium dichromate?
Determine the molar mass.
1 mole of (NH4)2Cr2O7 = 2 N + 8 H + 2 Cr + 7 O
= 2(14.0g/mol)+ 8(1.0g/mol)+ 2(52.0g/mol)+ 7(16.0g/mol)
(NH4)2Cr2O7 = 252.0 g/mol
(NH4)2Cr2O7
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Calculating MolesAnd the Factor Label Line
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The Factor Label line is used to organize calculations, ratios, and to choose the right units for the answer.
Rules for using a Factor Label Line
1. Start with what you know2. Put the unit you want to get rid of on the bottom3. Put the unit you want on the top4. Multiply across the top, Divide across the bottom
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What is the mass of 1.20 x 10–5 moles of carbon tetrachloride, CCl4?
CCl4 = 1 C + 4 Cl = 1(12.0 g/mol) + 4(35.5 g/mol) = 154.0 g/mol
or154.0 g1 mole
1.20 x 10-5 mol 1 mol
154.0 g
154.0 g1 mole
1.85 x 10-3 g
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1. 5.00 moles of aluminum atoms.2. 100.0 g of sugar, C11H22O11
3. 7.25 moles of iron (III) oxide.4. 1.42 x 10-3 g of copper (II) sulphate.
1. Al = 27.0 g/mol = 135 g 2. C11H22O11 = 330.2 g/mol = 0.303 mol3. Fe2O3 = 159.6 g/mol =1160 g 4. CuSO4 = 159.6 g/mol = 8.90 x 10-6
mol
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Calculating the Number of Particles
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One mole of anything contains 6.02×1023 individual particles.
The term "particles" refers to any individual thing like atoms, formula units, molecules, ions, etc.
or6.02 x 10 23 particles 1 mole 6.02 x 10 23 particles
1 mole
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How many atoms in 25.0 moles of copper?
25.0 mol Cu1.51 x 10 25 atoms=
How many molecules of water in 1.50 x 10–5 moles?
= 9.03 x 10 18 molecules of water
1.50 x 10–5 mol H2O
6.02 x 10 23 particles
1 mole
6.02 x 10 23 particles
1 mole
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How many moles is 5 atoms of zinc?
5 atoms of Zinc is 8.31 x 10–24 moles.
5 atoms Zn= 8.31 x 10-24 moles
6.02 x 10 23 particles
1 mole
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The mole allows the conversion between mass and number of particles.
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How many molecules of water in a 10.0 g sample of water?
0.556 mol H20=1 mole18.0 g
10.0 g H2O
0.556 mol H2O 6.02 x 10 23 particles
1 mole
= 3.34 x 10 23 molecules H20
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we can put the two equations together
There are 3.34 x 1023 molecules in 10.0 g of water.
1 mole6.02 x 10 23 particles of H2O10.0 g H2O
18.0 g1 mole
= 3.34 x 10 23 molecules H20
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How many atoms in 25.0 g of sodium chloride?
NaCl = 58.5 g/mol
= 5.14 x 10 23 atoms
1 mole6.02 x 10 23 For.U 25.0 g NaCl
58.5 g1 mole 2 atoms
1 For. U
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· The formula mass, in amu, is the sum of the atomic masses of all atoms in one substance.
· The molar mass of a substance is the mass of one mole of that substance, or its formula mass in grams.
· The mole is equal to 6.02 x 1023 particles -
Avogadro’s Number.
· Using molar mass, we can move between moles, mass, particles of a given substance.