Calculation of Empirical Formulas Empirical Formula consists of

  • Slides: 20
Download presentation

Calculation of Empirical Formulas • Empirical Formula = consists of the symbols for the

Calculation of Empirical Formulas • Empirical Formula = consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole number ratio • Molar mass= the mass in grams of 1 mole of a substance • this is the mass indicated for each element on the periodic table

Calculation of Empirical Formulas 1. treat percentages as a mass 2. Divide the given

Calculation of Empirical Formulas 1. treat percentages as a mass 2. Divide the given mass by the molar mass 3. Convert to whole numbers this can be done by dividing by the smallest number of moles If you still don’t have a whole number you can… Round to nearest whole number Multiple by 3 or 2 to get a whole number

Simplest formula calculations Q- a compound is found to contain the following % by

Simplest formula calculations Q- a compound is found to contain the following % by mass: 69. 58% Ba, 6. 090% C, 24. 32% O. What is the simplest (i. e. empirical) formula? Step 1: imagine that you have 100 g of the substance. Thus, % will become mass in grams. E. g. 69. 58 % Ba becomes 69. 58 g Ba. (Some questions will give grams right off, instead of %) Step 2: calculate the # of moles (mol = g ¸ g/mol) Step 3: express moles as the simplest ratio by dividing through by the lowest number. Step 4: write the simplest formula from mol ratios.

Simplest formula: sample problem Q- 69. 58% Ba, 6. 090% C, 24. 32% O.

Simplest formula: sample problem Q- 69. 58% Ba, 6. 090% C, 24. 32% O. What is the empirical (a. k. a. simplest) formula? 1: 69. 58 g Ba, 6. 090 g C, 24. 32 g O 2: Ba: 69. 58 g ¸ 137. 33 g/mol = 0. 50666 mol Ba C: 6. 090 g ¸ 12. 01 g/mol = 0. 50708 mol C O: 24. 32 g ¸ 16. 00 g/mol = 1. 520 mol O 3: Ba C O mol 0. 50666 0. 50708 0. 50666/ 0. 50708/ mol (reduced) 0. 50666 =1 = 1. 001 4: the simplest formula is Ba. CO 3 1. 520/ 0. 50666 = 3. 000

Mole ratios and simplest formula Given the following mole ratios for the hypothetical compound

Mole ratios and simplest formula Given the following mole ratios for the hypothetical compound Ax. By, what would x and y be if the mol ratio of A and B were: AB 3 A = 1 mol, B = 2. 98 mol A = 1. 337 mol, B = 1 mol A 4 B 3 A 7 B 3 A = 2. 34 mol, B = 1 mol A 2 B 3 A = 1 mol, B = 1. 48 mol 1. A compound consists of 29. 1 % Na, 40. 5 % S, and 30. 4 % O. Determine the simplest formula. 2. A compound is composed of 7. 20 g carbon, 1. 20 g hydrogen, and 9. 60 g oxygen. Find the empirical formula for this compound 3. - 6. Try questions 3 - 6 on page 189.

Question 1 1: Assume 100 g: 29. 1 g Na, 40. 5 g S,

Question 1 1: Assume 100 g: 29. 1 g Na, 40. 5 g S, 30. 4 g O 2: Na: 29. 1 g ¸ 22. 99 g/mol = 1. 266 mol Na S: 40. 5 g ¸ 32. 06 g/mol = 1. 263 mol S O: 30. 4 g ¸ 16. 00 g/mol = 1. 90 mol O 3: Na S O mol 1. 266 1. 263 1. 90 1. 266/ 1. 263/ 1. 90/ mol 1. 263 (reduced) = 1. 00 =1 = 1. 50 4: the simplest formula is Na 2 S 2 O 3 For instructor: prepare molecular models

Question 2 1: 7. 20 g C, 1. 20 g H, 9. 60 g

Question 2 1: 7. 20 g C, 1. 20 g H, 9. 60 g O 2: C: 7. 20 g ¸ 12. 01 g/mol = 0. 5995 mol C H: 1. 20 g ¸ 1. 01 g/mol = 1. 188 mol H O: 9. 6 g ¸ 16. 00 g/mol = 0. 60 mol O 3: C H O mol (reduced) 0. 5995/ 0. 5995 =1 1. 188/ 0. 5995 = 1. 98 4: the simplest formula is CH 2 O 0. 60/ 0. 5995 = 1. 0

Question 3 1: Assume 100 g: 28. 9 g K, 23. 7 g S,

Question 3 1: Assume 100 g: 28. 9 g K, 23. 7 g S, 47. 7 g O 2: C: 7. 20 g ¸ 12. 01 g/mol = 0. 5995 mol C H: 1. 20 g ¸ 1. 01 g/mol = 1. 188 mol H O: 9. 6 g ¸ 16. 00 g/mol = 0. 60 mol O 3: C H O mol 0. 5995 1. 188 0. 60 0. 5995/ 1. 188/ 0. 60/ mol 0. 5995 (reduced) 0. 5995 =1 = 1. 98 = 1. 0 4: the simplest formula is CH 2 O

Molecular formula calculations • There is one additional step to solving for a molecular

Molecular formula calculations • There is one additional step to solving for a molecular formula. First you need the molar mass of the compound. E. g. in Q 2, the molecular formula can be determined if we know that the molar mass of the compound is 150 g/mol. • First, determine molar mass of the simplest formula. For CH 2 O it is 30 g/mol (12+2+16). • Divide the molar mass of the compound by this to get a factor: 150 g/mol ¸ 30 g/mol = 5 • Multiply each subscript in the formula by this factor: C 5 H 10 O 5 is the molecular formula. (models) Q- For OF, give the molecular formula if the O 2 F 2 70 ¸ 35 = 2 compound is 70 g/mol

7. Combustion analysis gives the following: 26. 7% C, 2. 2% hydrogen, 71. 1%

7. Combustion analysis gives the following: 26. 7% C, 2. 2% hydrogen, 71. 1% oxygen. If the molecular mass of the compound is 90 g/mol, determine its molecular formula. 8. What information must be known to determine a) the empirical formula of a substance? b) the molecular formula of a substance? 9. A compound’s empirical formula is CH, and it weighs 104 g/mol. Give the molecular formula. 10. A substance is decomposed and found to consist of 53. 2% C, 11. 2% H, and 35. 6% O by mass. Calculate the molecular formula of the unknown if its molar mass is 90 g/mol.

Question 7 1: Assume 100 g total. Thus: 26. 7 g C, 2. 2

Question 7 1: Assume 100 g total. Thus: 26. 7 g C, 2. 2 g H, and 71. 1 g O 2: C: 26. 7 g ¸ 12. 01 g/mol = 2. 223 mol C H: 2. 2 g ¸ 1. 01 g/mol = 2. 18 mol H O: 71. 1 g ¸ 16. 00 g/mol = 4. 444 mol O 3: 2. 223 2. 18 4. 444 2. 223/2. 18/ 2. 18 4. 444/2. 18 = 1. 02 =1 = 2. 04 4: the simplest formula is CHO 2 5: factor = 90/45=2. Molecular formula: C 2 H 2 O 4

Question 8, 9 • For the empirical formula we need to know the moles

Question 8, 9 • For the empirical formula we need to know the moles of each element in the compound (which can be derived from grams or %). For the molecular formula we need the above information & the molar mass of the compound • Molar mass of CH = 13 g/mol Factor = 104 g/mol ¸ 13 g/mol = 8 Molecular formula is C 8 H 8

Question 10 1: Assume 100 g total. Thus: 53. 2 g C, 11. 2

Question 10 1: Assume 100 g total. Thus: 53. 2 g C, 11. 2 g H, and 35. 6 g O 2: C: 53. 2 g ¸ 12. 01 g/mol = 4. 430 mol C H: 11. 2 g ¸ 1. 01 g/mol = 11. 09 mol H O: 35. 6 g ¸ 16. 00 g/mol = 2. 225 mol O 3: 4. 430 11. 09 2. 225 4. 43/2. 225 11. 09/2. 225/2. 225 = 1. 99 = 4. 98 =1 4: the simplest formula is C 2 H 5 O 5: factor = 90/45=2. Molecular formula: C 4 H 10 O 2

Assignment 1. Calculate the percentage composition of each substance: a) Si. H 4, b)

Assignment 1. Calculate the percentage composition of each substance: a) Si. H 4, b) Fe. SO 4 2. Calculate the simplest formulas for the compounds whose compositions are listed: a) carbon, 15. 8%; sulfur, 84. 2% b) silver, 70. 1%; nitrogen, 9. 1%; oxygen, 20. 8% c) K, 26. 6%; Cr, 35. 4%, O, 38. 0% 3. The simplest formula for glucose is CH 2 O and its molar mass is 180 g/mol. What is its molecular formula?

4. Determine the molecular formula for each compound below from the information listed. substance

4. Determine the molecular formula for each compound below from the information listed. substance simplest formula molar mass(g/mol) a) octane C 4 H 9 114 b) ethanol C 2 H 6 O 46 c) naphthalene C 5 H 4 128 d) melamine CH 2 N 2 126 5. The percentage composition and approximate molar masses of some compounds are listed below. Calculate the molecular formula of each percentage composition molar mass(g/mol) 64. 9% C, 13. 5% H, 21. 6% O 74 39. 9% C, 6. 7% H, 53. 4 % O 60 40. 3% B, 52. 2% N, 7. 5% H 80

1 a) Si= 87. 43% (28. 09/32. 13 x 100), H= 12. 57% b)

1 a) Si= 87. 43% (28. 09/32. 13 x 100), H= 12. 57% b) Fe= 36. 77% (55. 85/151. 91 x 100), S= 21. 10% (32. 06/151. 91 x 100), O= 42. 13% 2 a) Assume 100 g. Thus: 15. 8 g C, 84. 2 g S. C: 15. 8 g ¸ 12. 01 g/mol = 1. 315 mol C S: 84. 2 g ¸ 32. 06 g/mol = 2. 626 mol S Mol reduced C 1. 315/1. 315 =1 the simplest formula is CS 2 S 2. 626/1. 315 = 2. 00

2 b) Ag: 70. 1 g ¸ 107. 87 g/mol = 0. 6499 mol

2 b) Ag: 70. 1 g ¸ 107. 87 g/mol = 0. 6499 mol Ag N: 9. 1 g ¸ 14. 01 g/mol = 0. 6495 mol N O: 20. 8 g ¸ 16. 00 g/mol = 1. 30 mol O Ag. NO 2 Ag N O Mol 0. 6499 0. 6495 1. 30 Mol. 6499/. 6495/. 6495 1. 30/. 6495 reduced = 1. 0 =1 = 2. 00 2 c) K: 26. 6 g ¸ 39. 10 g/mol = 0. 6803 mol K Cr: 35. 4 g ¸ 52. 00 g/mol = 0. 6808 mol Cr O: 38. 0 g ¸ 16. 00 g/mol = 2. 375 mol O K 2 Cr 2 O 7 K Cr O Mol 0. 6803 0. 6808 2. 375 Mol. 6803/. 6803. 6808/. 6803 2. 375/. 6495 reduced =1 = 1. 00 = 3. 49

3 C 6 H 12 O 6 (CH 2 O = 30 g/mol, 180/30

3 C 6 H 12 O 6 (CH 2 O = 30 g/mol, 180/30 = 6) 4 a) C 8 H 18 (C 4 H 9 = 57 g/mol, 114/57 = 2) b) C 2 H 6 O (C 2 H 6 O = 46 g/mol, 46/46 = 1) c) C 10 H 8 (C 5 H 4 = 64 g/mol, 128/64 = 2) d) C 3 H 6 N 6 (CH 2 N 2 = 54 g/mol, 126/42 = 3) 5 a) C: 64. 9 g ¸ 12. 01 g/mol = 5. 404 mol C H: 13. 5 g ¸ 1. 01 g/mol = 13. 37 mol H O: 21. 6 g ¸ 16. 00 g/mol = 1. 35 mol O C 4 H 10 O C H O Mol 5. 404 13. 37 1. 35 Mol 5. 404/1. 35 13. 37/1. 35/1. 35 reduced = 4. 00 = 9. 90 =1 C 4 H 10 O (C 4 H 10 O = 74 g/mol, 74/74 = 1)

5 b) C: 39. 9 g ¸ 12. 01 g/mol = 3. 322 mol

5 b) C: 39. 9 g ¸ 12. 01 g/mol = 3. 322 mol C H: 6. 7 g ¸ 1. 01 g/mol = 6. 63 mol H O: 53. 4 g ¸ 16. 00 g/mol = 3. 338 mol O CH 2 O C H O Mol 3. 322 6. 63 3. 338 Mol 3. 322/3. 322 6. 63/3. 322 3. 338/3. 322 reduced =1 = 2. 0 = 1. 00 C 2 H 4 O 2 (CH 2 O = 30 g/mol, 60/30 = 2) 5 c) B N H Mol 3. 728 3. 726 7. 43 Mol 3. 728/3. 726/3. 726 7. 43/3. 726 reduced = 1. 00 =1 = 2. 0 B 3 N 3 H 6 (BNH 2 = 26. 84 g/mol, 80/26. 84= 2. 98) For more lessons, visit www. chalkbored. com