Mole Concept. Conversion Factors:
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1 Today s focus.
2 Mole Concept Avogadro s Number is 6.02x10 23 The mole unit is used to express: 1. A mass quantity 2. A counting quantity 1 water molecule 1 mole of water molecules Conversion Factors: 6.02x10 23 amu = 1 gram (Scale up so that we can weigh in the lab) amu molecule 6.02x10 23 = 1 mole water molecules of water molecules g mole
3 Information in Chemical Formulae Sodium carbonate Na 2 CO 3 What are the parts needed to make ONE formula unit of sodium carbonate? Na C O
4 Information in Chemical Formulae Na 2 CO 3 Na : C : O 2 : 1 : 3
5 Information in Chemical Formulae Number of ratio of ions: (parts) Na 2 CO 3 2 : 1
6 Particles can be: # of atoms, Parts of a formula unit # of ions, # of molecules, # of formula units
7 Conversion Factor * Conversion Factor * * Conversion Factor * Particles can be: # of atoms, Parts of a formula unit # of ions, # of molecules, # of formula units *In a problem, look for unit given and unit sought.
8 Q: How many hydrogen atoms are in g of ammonium phosphate? (NH 4) 3PO 4 Dimensional Analysis: Unit given x conversion = unit sought factor(s) Do you expect the answer to be a big number or a small number? Conversion Factor: Molar Mass = g / mole 1mole x g ( NH 4) 3PO 4x (NH ) 41H atoms g (NH 4 ) 3 PO x =? H atoms (NH 4) 3PO 4. x 3mole 2PO A: 2.62x10 24 H atoms
9 Percent Composition (NH 4 ) 3 PO 4 This is an example of a theoretical calculation of Percent Composition of the elements in a the chemical formula. Formula Mass = g / mole Element Mass Contribution Percent Composition to the formula mass 42021g 1. Nitrogen x 3 = g / 14905mole x mole g. mole 1210g g1hydrogen x 12 = g / mole x mole. g mole1g. Phosphorus x 1 = g 905/ x mole mole g mole 6396g 1Oxygen x 4 = g / mole mole x. The percent composition of nitrogen in (NH 4 ) 3 PO 4 is %. etc. g mole 0= % = 8.118% = % = % 100%
10 Percent Composition Experimentally: Difference in mass = mass of oxygen + Start with KClO 3 of a certain mass After heating, solid remains should have less mass Oxygen escaped
11 Empirical Formula The simplest formula for a compound that has the SIMPLEST whole number ratio of the atoms present. Example: Water H 2 O H 2 O is the chemical formula of water. 2 : 1 Since this is the SIMPLEST whole number ratio of H:O. Therefore, H 2 O is also the empirical formula for water.
12 Empirical Formula The simplest formula for a compound that has the SIMPLEST whole number ratio of the atoms present. Example: Hydrogen peroxide H 2 O 2 H 2 O 2 is the chemical formula of hydrogen peroxide. 2 : 2 The chemical formula is NOT the SIMPLEST whole number ratio of H:O. Therefore, the empirical formula for hydrogen peroxide is HO.
13 Empirical Formula The simplest formula for a compound that has the SIMPLEST whole number ratio of the atoms present. Chemical formula H:O Empirical of the compound Ratio Formula H 2 O water Multiple 2:1 H 2 O 1x H 2 O :2 HO 2x hydrogen peroxide What do we know from this: 1. Sometimes the chemical formula IS the empirical formula, sometimes it is not. 2. The chemical formula IS a multiple of the empirical formula. When the chemical formula is the empirical formula, the multiple is one. 3. If we know the empirical formula and we know the molar mass of the compound, then we can determine the chemical formula of the compound!
14 From Empirical Formula to Chemical Formula Question: Hexane has a molar mass of g / mole. The empirical formula of hexane is C 3 H 7. What is the chemical formula of hexane? Chemical formula of the compound C:H Ratio Empirical Formula Multiple Hexane? 3:7 C 3 H 7 2 A: C 6 H 14 x2 Empirical formula has a mass of: ( x 3) + (1.008x7) = g / mole. 7To determine the multiple, 8molar mass of compound Multiple empirical formula mass. =2 05g mole g mole
15 Percent Composition Empirical Formula Chemical Formula Road Map
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17 61Question: A sample was sent to the lab and the analysis comes back showing us that the following mass percent of the elements was found. What is the empirical formula? 15.88% Carbon 2.22 % Hydrogen 63.42% Oxygen 18.50% Nitrogen Elements 100 g Moles of Elements Mole Ratio C g 15 = moles 18mole. g g x 3 = 3 H O N 2.22 g g g 22. g 10mole 08. g = moles Divide through. by the 3964smallest 3= moles 1320 number x 3 = 9 342mole. g g. 850mole. g = moles 1g x 3 = 3 x 3 = 5 Answer: C 3 H 5 O 9 N 3 (Nitroglycerine or TNT)
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19 Do the Percent Composition, Empirical Formula, Chemical Formula Worksheet. Answers will be posted later in the week. Try some practice problems in Maple TA. Use Dimensional Analysis in ALL your calculations!!
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