3.1 Percent Composition
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1 3.1 Percent Composition The percentage composition of a compound refers to the relative mass of each element in a compound. The Law of Definite Proportions states that the elements in a given chemical compound are always present in the same proportion by mass. Water Hydrogen Peroxide Oct 8 10:35 PM The mass of an element in a compound can be expressed as mass percent or PERCENTAGE COMPOSITION (the relative mass of each element in a compound expressed as percent). Calculating % Composition (2 types): 1. Given Compound Only 2. Given a Mass Sample {Bubble gum activity} Sep 30 7:43 PM 1
2 Example 1: A sample of a compound has a total mass of 48.72g. The sample is found to contain 32.69g of zinc and 16.03g of sulfur. What is the percent composition of the compound? Need to take the mass of zinc and divide it by the total mass Need to take the mass of sulfur and divide it by the total mass Oct 8 10:46 PM Example 2: A chemical has a total mass of g and is made up of C, O, and N. The sample contains 83.25g of carbon and 36.55g of O. Calculate the percent composition of each element. *Don't worry about sig figs...just put the percents to two decimal places! Oct 8 10:52 PM 2
3 Practice Problems page 82 #1 4 Oct 9 12:19 PM Practice Problems page 82 #1 4 Oct 8 10:55 PM 3
4 Calculating % Composition from a Formula Example 1: Determine the percent composition of aluminum hydroxide, Al(OH) 3. Oct 8 10:57 PM Example 2: a) Calculate the percent composition of iron (III) oxide. b) Calculate the mass of iron that could be extracted from a g sample of iron (III) oxide. Practice Problems page 85 #5 8 Oct 8 11:01 PM 4
5 Oct 11 9:37 AM Oct 15 8:41 AM 5
6 3.2 Empirical Formula The formula of a compound expressed as the smallest possible whole number ratio of subscripts of the elements in the formula. Molecular Formula Empirical Formula C 2 H 4 C 6 H 12 O 6 H 2 O C 2 H 6 H 2 O 2 C 3 H 4 Oct 15 8:44 AM Can different compounds have the same empirical formula? Example: Benzene C 6 H 6 Ethyne C 2 H 2 Oct 15 8:47 AM 6
7 Note: Ionic compounds DO NOT have molecular formulas. *They exist as a ratio of ions. *The empirical formula of an ionic compound is usually the same as its chemical formula. Oct 15 8:49 AM Steps to Finding Empirical Formula Percent to mass Mass to mole Divide by small Multiply til'whole Oct 15 8:52 AM 7
8 Example 1: Calculate the empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen. Oct 15 8:55 AM What would you multiply by to get a whole number? Oct 15 9:28 AM 8
9 Example 2: Determine the empirical formula of a compound that has 80.2% carbon, 9.62% hydrogen and 10.2% oxygen. Oct 15 9:43 AM Example 3: Calculate the empirical formula of a compound containing 11.2g of iron and 21.3g of chlorine. Oct 15 9:52 AM 9
10 Example 4: Calculate the empirical formula of a compound that is 85.6% carbon and 14.4% hydrogen. Oct 15 9:59 AM Practice Problems page 89 #9 12 page 91 #13 16 page 94 #2,4,6,7 Oct 15 10:00 AM 10
11 Exit Pass What is the empirical formula of a compound that contains 67.6% mercury, 10.8% sulfur, and 21.6% oxygen? Oct 15 1:22 PM Determining the Empirical Formula of a Hydrate *Many ionic compounds crystallize from a water solution with water molecules incorporated into their structure. This is called a hydrate. Oct 21 7:49 AM 11
12 Every hydrate has a specific number of water molecules bonded to each formula unit. MgSO 4 7H 2 O CaSO 4 2H 2 O Ba(OH) 2 8H 2 O CaCl 2 6H 2 O Fe(OH) 2 3H 2 O *You need to remember the prefixes! Oct 21 7:57 AM Calculations Example 1: A 50.0g sample of a hydrate of barium hydroxide, Ba(OH) 2, contains 27.2g of Ba(OH) 2. Find the value of x in Ba(OH) 2 xh 2 O. Oct 21 8:01 AM 12
13 Example 2: A 3.34g sample of a hydrate has the formula SrS 2 O 3 xh 2 O and contains 2.30g of SrS 2 O 3. Find the formula of the hydrate. Oct 21 8:04 AM Example 3: The mass of water in a hydrate of MnCl 2 xh 2 O is 36.4g.The total mass of the hydrate is 100g. What is the empirical formula of the hydrate? Oct 21 8:08 AM 13
14 Example 4: A hydrate of zinc nitrate has the formula Zn(NO 3 ) 2 xh 2 O. If the mass of 1 mol of the anhydrous zinc nitrate is 63.67% of the mass of 1 mol of the hydrate, what is the value of x? Oct 21 8:13 AM Example 5: A 9.00g sample of calcium phosphate tetrahydrate was thoroughly heated to remove all the water of hydration. What is the mass of the anhydrous calcium phosphate? Oct 21 8:15 AM 14
15 Practice Problems page 108 #21 Oct 21 8:20 AM 3.3 Molecular Formula Suppose a suspect in a theft investigation is a researcher in a biology laboratory. The suspect works with formaldehyde, CH 2 O. Police officers find traces of a substance at the crime scene and send samples to the Centre for Forensic Science. The forensic analysts find that the substance contains a compound that has an empirical formula CH 2 O. Will this evidence help to convict the suspect? Oct 29 8:40 AM 15
16 Name Molecular Formula Empirical Formula formaldehyde CH 2 O CH 2 O acetic acid C 2 H 4 O 2 lactic acid C 3 H 6 O 3 erythrose C 4 H 8 O 4 ribose C 5 H 10 O 5 glucose C 6 H 12 O 6 Oct 29 8:46 AM Determining a Molecular Formula Steps: 1. Find EF 2. Find molar mass of EF 3. Molar mass of molecular formula (usually given in question) Molar mass of EF 4. Multiply EF by answer to #3 Oct 29 8:50 AM 16
17 Example 1: The empirical formula of ribose is CH 2 O, with a molar mass of 150g/mol. What is the molecular formula? Oct 29 8:53 AM Example 2: Determine the molecular formula of capsaicin if it contains 71% carbon, 8% hydrogen, 15.8% oxygen and 14% nitrogen with a molar mass 304g/mol. Oct 29 9:14 AM 17
18 Example 3: The empirical formula of a certain dioxin is C 6 H 2 OCl 2. If the molar mass of the dioxin is 322g/mol, what is the molecular formula? Oct 29 9:29 AM Practice Problems page 97 #17,18,19 Oct 29 9:31 AM 18
19 The Carbon Hydrogen Combustion Analyzer C x H y + O 2 CO 2 + H 2 O A large number of important chemicals are composed of H, C, and O. The carboncombustion analyzer is a useful instrument for analyzing these chemicals. (see diagram on page 99) Oct 29 10:47 AM After the combustion, all the carbon in the sample is contained in the carbon dioxide and all the hydrogen in the sample is contained in the water. Oct 29 10:53 AM 19
20 Example 1: A 1.000g sample of a pure compound containing only carbon and hydrogen was combusted in a carbon hydrogen combustion analyzer. The combustion produced g of water and 3.338g of carbon dioxide. Determine the empirical formula. Oct 29 10:56 AM page 101 #22 Practice page 101 #21 Oct 29 10:59 AM 20
21 Work on EF of a hydrate lab If completed, start chapter 3 worksheet Oct 30 9:41 AM Review Worksheet on EF and MF page #6 #11 #12 #14 Combustion of a 1.086g sample containing carbon and hydrogen is burned in a carbonhydrogen combustion analyzer. 2.76g of CO 2 and 2.97g of H 2 O is produced. What is the empirical formula of the compound? C 4 H 21 Nov 4 8:57 AM 21
23 carbon atoms The number is known as Avogadro s d Number.
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