bellwork solve the following using dimensional analysis and place the answer in scientific notation....
TRANSCRIPT
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Bellwork
Solve the following using dimensional analysis and place the answer in scientific notation.
1. Jamie has 2.5 liters of mercury in a jar. What is the mass of this mercury if its density is 13.6 g/ml?
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The mole (mol) is one of the
seven base units in the SI system.
It measures the amount of
substance.
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The form in which a substance exists is its “representative particle”.Representative particles can be atoms, ions, molecules, formula units, or anything else.
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Just as one dozen is 12 representative particles of eggs, a mole is 6.02 x 1023 representative particles.
602,000,000,000,000,000,000,000!!!!!
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Examples:1 mole Fe = 6.02 x 1023 atoms of Fe
1 mole H2O molecules = 6.02 x 1023 molecules of water
1 mole NaCl formula units = 6.02 x 1023 NaCl formula units
1 mole eggs = 6.02 x 1023 eggs
You can have a mole of ANYTHING!!
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6.02 X 1023 Watermelon Seeds: Would be found inside a melon slightly larger than the moon.6.02 X 1023 Donut Holes: Would cover the earth and be 5 miles (8 km) deep.6.02 X 1023 Pennies:Would make at least 7 stacks that would reach the moon.6.02 X 1023 Grains of Sand: Would be more than all of the sand on Miami Beach.6.02 X 1023 Blood Cells: Would be more than the total number of blood cells found in every human on earth.
How much is a mole?
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Question
• How many molecules would be in 3 moles of water?
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Diatomic ElementsCertain elements are only stable in pairs or with other elements in a compound. These elements are called the diatomic elements.
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There are 7 diatomic elements:
Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, and Fluorine
(Memory trick: HBrONClIF or 7th Heaven)
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Avogadro’s Number
*6.02 x 1023 is called Avogadro’s number. *It is named after Amadeo Avogadro who did work in the 1800’s that allowed 6.02 x 1023 to be calculated.
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The mole is the “chemist’s dozen”. It is a convenient way to count extremely large numbers of atoms, molecules or ions.
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New Conversion Factor! 1 mole = 6.02 x 1023 representative particles
We work these problems using dimensional analysis.
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How many moles are 1.20 x 1025 atoms of phosphorous?
1.20 x 1025 atoms P 1 mol P 6.02 x 1023 atoms
= 19.9 mol P
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How many atoms are in 0.750 mol of Zn?
0.750 mol Zn 6.02 x 1023 atoms Zn = 1 mol Zn
4.52 x 1023 atoms Zn
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How many molecules are in 0.400 mol N2O5?
0.400 mol N2O5 6.02 x 1023molecules = 1 mole N2O5
2.41 x 1023 molecules
Q: What did Avogadro teach his students in math class?
A: Moletiplication
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How many moles are contained in 1.20 x 1024 molecules CO2?
1.20 x 1024 molec CO2 1 mol CO2
6.02 x 1023 molecules
= 1.99 moles CO2
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Question
• Your friend gives you a gold ring that contains 2.3 mol of atoms. How many atoms is this?
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Gram atomic mass (gam) -atomic mass of an element in grams-mass of one mole of atoms of a monatomic element
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Question
• Write the atomic masses of the following.
• Mg __________
• Cl ___________
• Ba ___________
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Example:C =12.0 g = mass of 6.02 x 1023atoms 12.0 g/mol is the gram atomic mass of carbon
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•Molar mass (M.M.) is a term used to describe the mass of a mole of a chemical compound.
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Molar Mass (M.M.)-mass of one mole of any compound-sum of the atomic masses of each atom in the compound
1 mol H2O: 2 mol H 1 mol O
=2 mol H x 1.008 g H/mol = 2.016 g =1 mol O x 15.999 g O/mol= 15.999 g 18.015 g H2O
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Question
• What is the gram molecular mass of P2O5?
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What is the molar mass of CH3OH?
C 1 x 12.011 = 12.011H 4 x 1.008 = 4.032O 1 x 15.999 = 15.999 32.042 g
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Quiz day
• Get ready for your quiz!!!
• Test on Wednesday!
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What is the M.M. of magnesium phosphate?
Mg3(PO4)2
3 mol Mg 3 x 24.305 g = 72.915 g
2 mol P 2 x 30.974 g = 61.948 g
8 mol O 8 x 15.999 g =127.992 g
262.855 g
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What is the molar mass of ammonium sulfate?
(NH4)2SO4
2 mol N 2 x 14.007 = 28.014 8 mol H 8 x 1.008 = 8.064 1 mol S 1 x 32.066 = 32.066 4 mol O 4 x 15.999 = 63.996 132.14 g
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Mole – Mass Conversions
New Conversion factor!
1 mol = molar mass ( grams)
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Find the mass in grams of 3.32 mol of K.
3.32 mol K 39.098 g K 1 mol K
= 1.30 x 102 g K
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Find the mass in grams of 15.0 mol of sulfuric acid.
H2SO4
H 2 x 1.008 = 2.016S 1 x 32.066 = 32.066O 4 x 15.999 = 63.996 98.078 g
15.0 mol H2SO4 98.078 g H2SO4
1 mol H2SO4
= 1470 g H2SO4
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Find the number of moles in 11.0 g of methane (CH4).
CH4 = (12.011g + 4.032g = 16.043 g)
11.0 g CH4 1 mol CH4
16.043 g CH4
= 0.686 mol CH4
What was Avogadro’s favorite Indian tribe?
The MOLEHICANS
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Bellwork
What is the molar mass of methane? Methane’s formula is CH4
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Molti-Step Mole Problems!
• Calculate the number of molecules present in 4.29 g of nitrogen dioxide (NO2).
• 4.29 g NO2 1 mol NO2 6.02x1023 m.c. NO2=
46.005 g NO2 1 mol NO2
= 5.61x1022 molecules NO2
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• Calculate the number of moles of sulfur atoms present in 2.01 g of sodium sulfide (Na2S).
• 2.01 g Na2S 1 mol Na2S 1 mol S atoms
78.046 g Na2S 1 mol Na2S
= 0.0258 mol S atoms
Molti-Step Mole Problems!
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• Calculate the mass in grams of 2.49 x 1020 carbon dioxide (CO2) molecules.
2.49 x 1020 CO2 m.c. 1 mol CO2 44.009 g CO2
6.02x1023 m.c.CO2 1 mol CO2
= 1.82 x 10-2 grams CO2
Molti-Step Mole Problems!
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• Calculate the grams of carbon in 12.2 mol sucrose, C12H22O11.
12.2 mol C12H22O11 12 mol C atoms 12.011 g C
1 mol C12H22O11 1 mol C atoms
= 1.76 x 103 g carbon
Molti-Step Mole Problems!
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Question
• Write the two conversion factors we have discussed below. Show how they are related.
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Molar Volume of a GasThe volume of a gas is usually measured at 0oC and 1 atmosphere of pressure.
This is called standard temperature and pressure (STP).
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-At STP, one mole of any gas has a volume of 22.4 L which is called the molar volume of a gas and contains 6.02 x 1023 particles of the gas.
-22.4 L of a gas has a mass equal to the gfm of the gas.
-So…1 mol = 22.4L = 6.02 x 1023 particles = M.M.
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New conversion factor!
1 mol of any gas at STP = 22.4 L
(for gases only)
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What is the volume (liters) at STP of 0.960 mol of methane, CH4?
0.960 mol CH4 22.4 L CH4
1 mol CH4
=21.5 L CH4
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At STP, how many moles are in 0.542 mL of neon gas?
0.542 mL Ne 1 L Ne 1 mol Ne 1000 mL Ne 22.4 L Ne
= 2.42 x 10-5 mol Ne
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Question
• Relate the three conversion factors we have learned below.
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Bellwork
• Jake has a jar full of sodium hydrogen carbonate, or baking soda (NaHCO3). What is the mass of 2.78 mol baking soda?
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Bellwork
• How many propane molecules are in 25.00 g of propane, C3H8?
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Percent Composition(remember: percent = part divided by total x 100)
percent by mass of each element in a compound
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What is the percent composition of NO2?
NO2
N 1 x 14.007 = 14.007 O 2 x 15.999= 31.998
( /46.005g)x100 =30.4%Ca
( /46.005g)x100 =69.6% C
46.005 100%
As long as your % adds up to 99-101% you are fine.
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Why is Avogadro so rich!
Because he is a multi-mole-ionairre!!!!
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What is the percent composition of calcium acetate?
Ca(C2H3O2)2
Ca1 x40.078=40.078C 4 x12.011=48.044H 6 x 1.008= 6.048O 4 x15.999=63.996 158.166 g
( /158.166g)x100=25.3% Ca( /158.166g)x100=30.4% C( /158.166g)x100=3.8% H( /158.166g)x100=40.5% O 100.0%
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Calculate the number of grams of calcium in 9.7 g of calcium acetate?
Ca(C2H3O2)2Ca 25.4%C 30.4%H 3.8%O 40.5%
9.7 g Ca(C2H3O2)2
100 g Ca(C2H3O2)2
25.4 g Ca = 2.46 g Ca
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Bellwork
• Susannah has 12.5g of HC2H3O2, or vinegar. How many MOLECULES of vinegar does she have?
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CALCULATING EMPIRICAL FORMULAS
Empirical formula - lowest whole number ratio of the elements in a compound- may or may not be the same as the molecular formula.
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Steps to calculate empirical formula:1. Find moles of each element.2. Set up mole ratio.3. Simplify mole ratio (divide by smallest). If your answers are not in whole numbers, you must multiply by 2,3,4,or 5 to get whole numbers.4. Use mole ratio as subscripts in the formula. If given % composition, assume 100 g of compound.
Empirical Formula Poem
Percent to mass,
mass to moles,
divide by smallest and
round ‘till whole!
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A compound is 79.8% C and 20.2% H. Find its empirical formula.
79.8gC 1mol C = 6.65 mol C 12.011 g C 20.2 g H 1 mol H = 20.0 mol H 1.008 g H
CH3
/6.65 = 1
/6.65 = 3
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Find the empirical formula for a compound made up of 26.7% P, 12.1% N and 61.2% Cl.
26.7 g P 1 mol P = 0.862 mol P 30.974 g P
12.1 g N 1 mol N = 0.864 mol N 14.007 g N
61.2 g Cl 1 mol Cl = 1.73 mol Cl
35.453 g Cl
/0.862=1
/0.862=1
/0.862=2
Empirical Formula = PNCl2
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Bellwork
• NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O. Calculate the empirical formula of NutraSweet.
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Molecular formulas are the actual formulas. They may be the same as the empirical formula or a multiple of it.
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To find the multiple (n), take the molar mass (M.M.) and divide by the empirical formula mass (efm):
n = M.M. efm
Multiply each subscript in the empirical formula by n to get the molecular formula.
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A white powder is analyzed and found to have the empirical formula P2O5. The compound has a molar mass of 283.9 g. What is the compound’s molecular formula?
P2O5 = 141.898 g/mol
M.M./efm
283.9 g/mol141.898 g/mol = 2
2(P2O5) = P4O10
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A compound used as an additive for gasoline to help prevent engine knock shows the following percentage composition: 71.65% Cl 24.27% C 4.07% HThe molar mass is known to be 98.96 g. Determine the empirical formula and the molecular formula for this compound.
71.65 g Cl 1 mol Cl = 2.02 mol Cl 35.453 g Cl24.27g C 1 mol C = 2.02 mol C 12.011 g C4.07g H 1 mol H = 4.04 mol H 1.008 g H
1:1:2 ClCH2 or CH2Clefm = 12.011+2.016+35.453=49.48
g/mol98.96/49.48=2 C2H4Cl2
/2.02 = 1
/2.02 = 1
/2.02 = 2
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Hydration
• Water of hydration – water in a crystal– When copper (II) sulfate is
dissolved in water and then the water allowed to evaporate, copper (II) sulfate pentahydrate is formed
– CuSO4 + 5H2O ↔ CuSO45H2O
• Hydrate - compound that contains water of hydration
The picture above shows copper (II) sulfate pentahydrate. Notice the water molecules surrounding the copper molecules.
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Hydration
• When cobalt (II) chloride is dissolved in water and then the excess water is allowed to evaporate, cobalt (II) chloride hexahydrate is formed
↔ CoCl2 6H2O CoCl2 + 6H2O
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In the hydrate CuSO4.5H20, how
many water molecules would be present in 3 formula units?
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Naming Hydrates
• To name a hydrate, use the following:– They are named by giving the name of the salt
followed by a prefix that stands for the number of water molecules associated with a formula unit of the salt.
• Ex: CuSO4 • 5H2O
copper (II) sulfate pentahydrate
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Bellwork
• How many moles of each substance are contained in the following samples? Be sure to include the correct units and sig figs in your answers.
• a) 6.0 x 1020 molecules of carbon dioxide
• b) 7.409 x 1013 molecules of water
• c) 5 x 1046 molecules of methane (CH4)
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Bellwork
• You have 10.0 g of aluminum and 73.0 g of gold. Which sample contains more total atoms, the aluminum or gold?
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Bellwork
• What is the molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen and 48.68% fluorine if the molar mass of this compound is 156.12 g?
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Bellwork
• What is the empirical formula for a compound that contains 17.34% hydrogen and 82.66% carbon?