ࡱ> )+&'({ bjbj`` ;ff:JJJdJ+jf6Maa<#b >i@i@i@i@i@i@i$lnLdiJ0cVr Ma0c0cdi?9iccc0cF<J>ic0c>icc|cԖ^ vc4c*ii0+jcoc(ocoJcHCb"ebc}bbCbCbCbdidicCbCbCb+j0c0c0c0coCbCbCbCbCbCbCbCbCbX X: Name Class Date 16. The figure below shows how to convert from one unit to another unit. Write the missing conversion factors below.  a. c. b. d.  10.3 Percent Composition and Chemical Formulas  A molecular formula of a compound is a whole-number multiple of its empirical formula. Lesson Summary Percent Composition of a Compound Percent composition is the percent by mass of each element in a compound. To find the percent by mass of an element in a compound, use the formula:  EMBED Equation.DSMT4  To find the mass of an element in a sample of a compound, use the formula:  EMBED Equation.DSMT4  Empirical Formulas The empirical formula of a compound is the formula with the smallest whole-number mole ratio of the elements. An empirical formula may or may not be the same as the actual molecular formula. 135 Name Class Date Molecular Formulas A molecular formula specifies the actual number of atoms in each element in one molecule or formula unit of the substance. To find a molecular formula, the molar mass of the compound must be determined. After reading Lesson 10.3, answer the following questions. Percent Composition of a Compound 1. How do you express relative amounts of each element in a compound? 2. Circle the letter of the phrase that completes this sentence correctly. The number of percent values in the percent composition of a compound is a. half as many as there are different elements in the compound. b. as many as there are different elements in the compound. c. twice as many as there are different elements in the compound. 3. What is the formula for the percent by mass of an element in a compound? 4. In the diagram below, which compound has a greater percent composition of chromium? How many more percentage points is this?    5. To calculate the percent composition of a known compound, start with the chemical formula of the compound and calculate the , which gives the mass of one mole of the compound. 6. Is the following sentence true or false? You can use percent composition to calculate the number of grams of an element in a given amount of a compound. 7. How do you calculate the grams of an element in a specific amount of a compound? 136 Name Class Date Empirical Formulas 8. An empirical formula of a compound gives the whole-number ratio of the atoms of the elements in a compound. 9. Is the following sentence true or false? The empirical formula of a compound is always the same as the molecular formula. 10. Look at Figure 10.11 and Table 10.3. Name three compounds that have an empirical formula of CH. 11. Fill in the labels on the diagram below.      Molecular Formulas 12. The molecular formula of a compound is either the same as its empirical formula or a of it. 13. What do you need to know to calculate the molecular formula of a compound? 14. If you divide the molar mass of a compound by the empirical formula mass, what is the result? 15. What factor would you use to convert the empirical formula of a compound to a molecular formula? 137 Name Class Date Guided Practice Problems Answer the following questions about Practice Problem 1. If 0.20 bushel is 1 dozen apples and a dozen apples has a mass of 2.0 kg, what is the mass of 0.50 bushel of apples? Analyze Step 1. List the knowns and the unknown. KnownsUnknown     Use dimensional analysis to convert the number of bushels to the mass of apples, by following this sequence of conversions: number of bushels ! dozens of apples ! mass of apples Calculate Step 2. Solve for the unknown. The first conversion factor is . The second conversion factor is . Multiplying the number of bushels by these two conversion factors gives the answer in kilograms. The mass of 0.50 bushel of apples is . Evaluate Step 3. Does the result make sense? 138 Name Class Date Answer the following questions about Practice Problem 3. How many moles is 2.80 1024 atoms of silicon? Step 1. List what you know. 2.80 1024 atoms of Si atoms in one mole Step 2. Multiply the atoms of silicon by a mol/atoms conversion factor.  EMBED Equation.DSMT4   Step 3. Divide. mol Answer the following questions about Practice Problem 5. How many atoms are in 1.14 mol of sulfur trioxide (SO3)? Analyze Step 1. List the knowns and the unknown. Knowns Unknown Calculate Step 2. Solve for the unknown. The first conversion factor is EMBED Equation.DSMT4  The second conversion factor is EMBED Equation.DSMT4  Multiply moles of SO3 by these conversion factors:  = Evaluate Step 3. Does the result make sense? 139 Name Class Date Answer the following questions about Practice Problem 7. Find the molar mass of PCl3. Analyze Step 1. List the knowns and the unknown. KnownsUnknown    Calculate Step 2. Solve for the unknown. Convert moles of phosphorus and chlorine to grams of phosphorus and chlorine. Then add to get the results.  molar mass of PCl3 = Evaluate Step 3. Does the result make sense? Answer the following questions about Practice Problem 16. Find the mass, in grams, of 4.52 10"3 mol C20H42. Analyze Step 1. List the known and the unknown. KnownUnknown    140 Name Class Date Calculate Step 2. Solve for the unknown. Determine the molar mass of C20H42: 1 mol C20H42 = 20 12.0 g + 42 1.0 g = 282 g Multiply the given number of moles by the conversion factor:  Evaluate Step 3. Does the result make sense? Answer the following questions about Practice Problem 18. Find the number of moles in 3.70 10"1 g of boron. Analyze Step 1. List the known and the unknown. KnownUnknown  The unknown number of moles is calculated by converting the known mass to the number of moles using a conversion factor of mass ! moles. Calculate Step 2. Solve for the unknown. Determine the molar mass of boron: 1 mol B = 10.8 g B Multiply the given mass by the conversion factor relating mass of boron to moles of boron:  Evaluate Step 3. Does the result make sense?   141 Name Class Date Answer the following questions about Practice Problems 20a and 20b. What is the volume of these gases at STP? a. 3.20 10"3 mol CO2 b. 3.70 mol N2 3.20 10"3 mol CO2 Analyze Step 1. List the knowns and the unknown. KnownsUnknown   To convert moles to liters, use the relationship 1 mol CO2 = 22.4 L CO2 (at STP). Calculate Step 2. Solve for the unknown. Multiply the given number of moles of CO2 by the conversion factor:  Evaluate Step 3. Does the result make sense? 3.70 mol N2 Analyze Step 1. List the knowns and the unknown. KnownsUnknown   Use the relationship 1 mol N2 = 22.4 L N2 (at STP) to convert moles to liters. 142 Name Class Date Calculate Step 2. Solve for the unknown. Multiply the given number of moles of N2 by the conversion factor:  Evaluate Step 3. Does the result make sense? Answer the following questions about Practice Problem 22. A gaseous compound composed of sulfur and oxygen has a density of 3.58 g/L at STP. What is the molar mass of this gas? Analyze Step 1. List the knowns and the unknown. KnownsUnknown    To convert density (g/L) to molar mass (g/mol), a conversion factor of L/mol is needed. Calculate Step 2. Solve for the unknown. Multiply the density by the conversion factor relating liters and moles:  EMBED Equation.DSMT4  Evaluate Step 3. Does the result make sense? 143 Name Class Date Answer the following questions about Practice Problem 33. A compound is formed when 9.03 g Mg combines completely with 3.48 g N. What is the percent composition of this compound? Analyze Step 1. List the knowns and the unknowns. Knowns Unknowns The percent of an element in a compound is the mass of the element in the compound divided by the mass of the compound. To be expressed as a percentage, the ratio must be multiplied by 100%. Calculate Step 2. Solve for the unknown.  EMBED Equation.DSMT4   EMBED Equation.DSMT4  Evaluate Step 3. Does the result make sense? 144 Name Class Date Answer the following questions about Practice Problem 36. Calculate the percent composition of these compounds. a. ethane (C2H6) b. sodium hydrogen sulfate (NaHSO4) Ethane (C2H6) Analyze Step 1. List the knowns and the unknowns. Knowns Unknowns Because no masses are given, the percent composition can be determined based on the molar mass of the substance. The percent of an element in a compound is the mass of the element in the compound divided by the mass of the compound. To express the ratio as a percent, the ratio is multiplied by 100%. Calculate Step 2. Solve for the unknown.  EMBED Equation.DSMT4   EMBED Equation.DSMT4  Evaluate Step 3. Does the result make sense? 145 Name Class Date Sodium hydrogen sulfate (NaHSO4) Analyze Step 1. List the knowns and the unknowns. Knowns Unknowns Because no masses are given, the percent composition can be determined based on the molar mass of the substance. The percent of an element in a compound is the mass of the element in the compound divided by the mass of the compound. To express the ratio as a percent, the ratio is multiplied by 100%. Calculate Step 2. Solve for the unknown.  EMBED Equation.DSMT4   EMBED Equation.DSMT4   EMBED Equation.DSMT4   EMBED Equation.DSMT4  Evaluate Step 3. Does the result make sense? 146 Name Class Date Answer the following questions about Practice Problem 39. Calculate the empirical formula of each compound. a. 94.1% O, 5.9% H b. 67.6% Hg, 10.8% S, 21.6% O 94.1% O, 5.9% H Analyze Step 1. List the knowns and the unknown. Knowns Unknown Use the percent composition to convert to mass, recalling that percent means parts per hundred. Then use the molar mass to convert to number of moles. Finally, determine whole-number ratios based on the number of moles of each element per 100 grams of compound. Calculate Step 2. Solve for the unknown. One hundred grams of compound has 5.9 g H and 94.1 g O. Multiply by conversion factors relating moles of the elements to grams:  So, the mole ratio for 100 g of the compound is H5.9O5.9. But formulas must have whole number subscripts. Divide each molar quantity by the smaller number of moles. This will give 1 mol for the element with the smaller number of moles. In this case, the ratio is 1:1, so the empirical formula is simply H1O1. However, a subscript of 1 is never written, so the answer is . Evaluate Step 3. Does the result make sense? 147 Name Class Date 67.6% Hg, 10.8% S, 21.6% O Analyze Step 1. List the knowns and the unknown. Knowns Unknown Use the percent composition to convert to mass. Then use molar mass to convert to number of moles. Finally, determine whole-number ratios based on the number of moles of each element per 100 grams of compound. Calculate Step 2. Solve for the unknown. One hundred grams of compound has 67.6 g Hg, 10.8 g S, and 21.6 g O. Multiply by a conversion factor relating moles to grams:  So, the mole ratio for 100 g of the compound is Hg0.34S0.34O1.35. Divide each molar quantity by the smaller number of moles:  EMBED Equation.DSMT4   EMBED Equation.DSMT4   EMBED Equation.DSMT4  The empirical formula is . 148 Name Class Date Evaluate Step 3. Does the result make sense? Answer the following questions about Practice Problem 42. Find the molecular formula of ethylene glycol, which is used as antifreeze. The molar mass is 62.0 g/mol and the empirical formula is CH3O. Analyze Step 1. List the knowns and the unknown. Knowns Unknown Calculate Step 2. Solve for the unknown. First, calculate the empirical formula mass (efm):  So, efm = 12 g + 3 g + 16 g = 31 g. Divide the molar mass by the empirical formula mass: Molar mass/efm = 62 g/31 g = 2 Multiply subscripts in the empirical formula by this value. The molecular formula is . Evaluate Step 3. Does the result make sense? 149 Name Class Date  A student has a sample of CO2 gas that has a mass of 22.0 g. a. Explain how she would find the volume of the sample at STP. b. What is the volume of 22.0 g of CO2 at STP? Show your work. 150 Name Class Date  For Questions 19, complete each statement by writing the correct word or words. If you need help, you can go online. 10.1 The Mole: A Measurement of Matter 1. Knowing how the , mass, and volume of an item relate to a common unit allows you to convert among these units. 2. Counting the representative particles in a sample of a substance is based on the . 3. The molar mass of an element is its expressed in units of grams. 4. The molar mass of a(n) is the sum of the molar mass of all the elements in the . 10.2 Mole-Mass and Mole-Volume Relationships 5. The of a substance is used to convert from mass to moles or moles to mass. 6. The of a gas is used to convert moles to volume or volume to moles at STP. 10.3 Percent Composition and Chemical Formulas 7. To find the percent by mass of an element in a compound, divide the mass of the element by the , then multiply by 100%. 8. The of a compound gives the lowest whole-number ratio of the atoms or moles of the elements in a compound. 9. 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Divide the mass of each element by the molar mass. b. Find the mass of each element in one mole of glucose. c. Multiply each quotient by 100%. d. Find the molar mass of glucose. EXTENSION Use the sequence you wrote to find the percent composition of glucose. Review Vocabulary For each term in column 1, write the letter of the best match from column 2. 1. mole 2. Avogadros number 3. representative particle 4. molar mass 5. 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