Chemical Formulas Percent Composition Empirical Formula Molecular Formula

Percentage Composition n the percentage by mass of each element in a compound of

Percentage Composition n Find the % composition of each element in Cu 2 S.

Percent Composition n Find the percent composition of each element in water. %H= 2

A. Percentage Composition n Find the percentage composition of a sample that is 28

A. Percentage Composition n How many grams of copper are in a 38. 0

A. Percentage Composition n Find the mass percentage of water in calcium chloride dihydrate.

B. Empirical Formula n Smallest whole number ratio of atoms in a compound C

B. Empirical Formula 1. Find mass of each element. If have %, then assume

B. Empirical Formula n Find the empirical formula for a sample of 25. 9%

B. Empirical Formula N 1 O 2. 5 Need to make the subscripts whole

C. Molecular Formula n “True Formula” - the actual number of atoms in a

C. Molecular Formula 1. Find the empirical formula. 2. Find the empirical formula mass.

C. Molecular Formula n The empirical formula for ethylene is CH 2. Find the

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Chemical Formulas Percent Composition Empirical Formula Molecular Formula I II III

Percentage Composition n the percentage by mass of each element in a compound of the element

Percentage Composition n Find the % composition of each element in Cu 2 S. 2 (63. 55 g) 100 = %Cu Cu = 79. 85% 159. 17 g Cu Cug 2 SS 32. 07 %S = 100 = 159. 17 g 20. 15% S Cu 2 S

Percent Composition n Find the percent composition of each element in water. %H= 2 (1. 01) g H 18. 02 g H 20 16. 00 g O %O= 18. 02 g H 2 O 100 = 11. 21 % H 100 = 88. 79 % S

A. Percentage Composition n Find the percentage composition of a sample that is 28 g Fe and 8. 0 g O. 28 g 100 = 78% Fe %Fe = 36 g %O = 8. 0 g 36 g 100 = 22% O

A. Percentage Composition n How many grams of copper are in a 38. 0 -gram sample of Cu 2 S? Cu 2 S is 79. 852% Cu (38. 0 g Cu 2 S)(0. 79852) = 30. 3 g Cu

A. Percentage Composition n Find the mass percentage of water in calcium chloride dihydrate. 36. 04 g %H 2 O = 100 =24. 51% H 2 O 147. 02 g

B. Empirical Formula n Smallest whole number ratio of atoms in a compound C 2 H 6 reduce subscripts CH 3

B. Empirical Formula 1. Find mass of each element. If have %, then assume out of 100 grams. 2. Convert the mass to moles of each element. 3. Divide moles by the smallest # to find subscripts. 4. When necessary, multiply subscripts by 2, 3, or 4 to get whole #’s.

B. Empirical Formula n Find the empirical formula for a sample of 25. 9% N and 74. 1% O. 25. 9 g 1 mol = 1. 85 mol N =1 N 1. 85 mol 14. 01 g 74. 1 g 1 mol = 4. 63 mol O = 2. 5 O 16. 00 g 1. 85 mol

B. Empirical Formula N 1 O 2. 5 Need to make the subscripts whole numbers multiply by 2 N 2 O 5

C. Molecular Formula n “True Formula” - the actual number of atoms in a compound empirical formula CH 3 ? molecular formula C 2 H 6

C. Molecular Formula 1. Find the empirical formula. 2. Find the empirical formula mass. 3. Divide the molecular mass by the empirical mass. 4. Multiply each subscript by the answer from step 3.

C. Molecular Formula n The empirical formula for ethylene is CH 2. Find the molecular formula if the molecular mass is 28. 1 g/mol? empirical mass = 14. 03 g/mol 28. 1 g/mol 14. 03 g/mol = 2. 00 (CH 2)2 C 2 H 4