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Drill: Calculate the % composition of each element in MgN 2 O 3
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CHM II HW Review PP 06 Work the problems attached to Poly’s website.
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Molar Conversions
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Moles The standard unit of measure for the amount of a substance in numbers
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Dozen = 12 of anything
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Moles = the amount of a substance that would = its mass in g from the PT
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Moles = 6.022 x 10 23 of anything
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Molar Conversions Mass to moles Volume of a gas to moles Particles to moles Volume of a solution to moles
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Moles First
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Mass to Moles Use atomic masses from the periodic table NaCl = 58.5 g/mole
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Gas Volume to Moles At STP: 22.4 L/mole Non-STP: PV = nRT PV RT n =
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Particles to Moles Use Avogadro’s Number 6.02 x 10 23 atoms, molecules, etc/mole
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Soln Volume to Moles Multiply molarity times volume n = M x V
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Solution Measures Molarity (M) = the number of moles of solute per liter of solution Others later
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Calculate the atomic mass of the element made up of the following isotopes: 99.50 % H-1 0.30 % H-2 0.20 % H-3
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Calculate the atomic mass of the element made up of the following isotopes: 5.0 % Pu-242, 5.0 % Pu-243 80.0 % Pu-244, & 10.0 % Pu-245
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Convert 7.0 g of silicon to moles
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Convert 250 g of CaCO 3 to moles
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Convert 3.0 moles of helium to grams
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Convert 11.2 L of oxygen gas at STP to moles
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Convert 0.20 moles of helium to volume at STP
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Convert: 2.0 x 10 24 atoms He to moles
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Convert 3.0 moles of glucose to molecules
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Convert 250 mL of 0.10 M HCl to moles
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Convert 6.8 g NH 3 to volume of gas at STP
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Drill: Determine the volume required to make 60.0 g NaOH into a 0.75 M solution
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Convert 3.0 x 10 25 molecules of CO 2 to mass in kg
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Drill: Calculate the number molecules in 32 g of Fe 2 O 3
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First Test Next Thursday on nomenclature, molar conversions, & reactions.
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Calculate the number of atoms in 16 ng of Fe 2 (SO 4 ) 3
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Empirical Formula
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Lowest whole number ratio of elements in a compound C 6 H 12 O 6 : EF = CH 2 O
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Determining Empirical formulas from percent composition
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Assume 100 g Change % directly to grams Use molar conversions to convert grams to moles Divide each molar amount by the smallest molar amount
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Find empirical for a compound with: 70.0 % Fe 30.0 % O
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Find empirical for a compound with: 40 % Ca 12 % C 48 % O
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Find empirical for a compound with: 40.0 % C 6.7 % H 53.3 % O
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Molecular Formula
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The actual whole number for each element in the compound
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Molecular Formula C 6 H 12 O 6 Empirical Formula CH 2 O
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Solving MF from EF 1) Solve empirical mass 2) Divide EM into MM 3) Multiply EF by quotient
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Drill: Calculate the mass of solute required to make 40.0 mL of 0.25 M Pb(NO 3 ) 2
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Test Review on Nomenclature, Molar conversions, & % Composition.
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Calculate the % composition of each element in Pb(NO 3 ) 2
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Calculate the empirical formula of a substance containing 62.7 % Po, 28.8 % O, & 8.4 % N.
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Calculate the molecular formula of a substance with an empirical formula of NH 2 & a molecular mass of 32 g/mole.
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Name each of the following: SeOMgS PbO 2 Cl 2 O KNO 3 ScCl 3
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Derive formulas for each: Cesium oxide Barium chloride Calcium phosphate Manganese(II) chlorate
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Name each of the following: NH 4 ClBaSO 4 KC 2 H 3 O 2 K 2 HPO 3 KNO 3 CuBrO Li 2 CO 3 MgC 2 O 4
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Name each of the following: HClH 2 SO 4 H 2 S H 3 PO 3 HNO 3 HBrO H 2 CO 3 HBrO 4
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Calculate the number of hydrogen atoms in 1.8 kg of PH 5.
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Calculate the volume at STP of 6.0 ng of NO.
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Calculate the mass of KBr required to make 250 mL of a 0.40 M solution.
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Chapter 3 General Define all the Key Terms on page 74
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Atomic Mass Work problems: 1 - 9 on page 75
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Avogadro’s Num. Work problems: 11 - 18 on page 75
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Molar Conversions Work problems: 18 - 26 on page 75 & 76
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% Composition Work problems: 27 - 34 on page 76
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Empirical Formula Work problems: 35 - 46 on page 76 & 77
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Balancing Rxns Work problems: 49 & 54 on page 77
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Stoichiometry Work problems: 55 & 64 on page 77 & 78
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Limiting Reactant Work problems: 65 & 74 on page 78 & 79
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