How many eggs are there in 5 dozen

How many eggs are there in 5 dozen? How many moles are in 2. 25 grams of the element iron, Fe?

Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221. Math. 1 Objective: The learner will convert the amount of a substance by using molar conversions through dimensional analysis.

Introduction to the Mole

What is a mole? Mole – SI base unit used to measure the amount of a substance What is molar mass? Molar mass – the mass in grams of one mole of a substance (ex. hydrogen 1. 0079 g/mol) What is the conversion factor for molar mass? 1 mole= mass of an atom (mass number)

Practice What is the number of moles found in 50. 4 grams of Uranium? Calculate the number of moles of 80. 850 g of nitrogen. Calculate the number of moles in 334 grams of lead.

Moles to Grams 6. 0 moles carbon= _____ grams carbon 4. 5 x 103 moles K = ______ grams K Determine the mass in grams of 19. 73 moles of the element boron, B.

8. 90 mol Ca = ______ g Ca 2. 8 mol Fe = ______ g Fe 4. 59 x 102 mol F = _______ g F 6. 000 mol S = ______ g S

PROVE IT!!!!!!!

5. 68 g N= ___ mol N

0. 405 mol N

0. 0821 mol Rb= ___ g Rb

7. 02 g Rb

3400 g O= ___ mol O

210 mol O

34. 71 mol As= ___ g As

2600. g As

Exit slip Determine the number of moles of 46. 3 grams of the element, copper, Cu? Evaluate and explain in words how you solve this problem. Tell me step by step in complete sentences (4 to 5 sentences).

Homework What is the mass in grams of. 375 mol of the element potassium, K. What is the mass in grams of 0. 0135 mol of the element, sodium, Na? How many moles of gold, Au, are in 3. 6 x 10 -10 g How many moles of copper, Cu, are in 3. 22 g of copper?

Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221. Math. 1 Objective: The learner will convert the amount of a substance by using Avogadro’s number through dimensional analysis.

Avogadro’s Number and Molar Conversions

Avogadro’s Number Avogadro was born in Italy from 1776 -1865 His field of study was physics. He developed Avogadro’s number which is 6. 022 x 10 23 6. 022 x 1023 = 1 mol

Moles to Avogadro’s Number 0. 30 mol of F = ______ atoms F. 2. 66 mol of N= ______ atoms N? How many atoms are in 4. 2 mol O?

Avogadro’s Number to Moles 6. 7 x 1026 atoms of Zn= _______ moles Zn 1. 69 x 1023 atoms of V= _______ moles V? How many moles are in 3. 29 x 1021 atoms Al?

Practice Please !!!!!! 0. 187 mol Ca = _____ atoms Ca How many atoms are in 1. 45 x 10 -17 moles of As? 5. 00 x 1021 atoms of S = _____ moles S How many moles of neon are in 7. 60 x 1024 atoms?

PROVE IT!!!!!!!

5. 68 g. N=__mol N

0. 0821 mol Rb=__g Rb

0. 187 mol. Ca=__atoms Ca

7. 60 x 1024 Ne atoms=___ moles Ne

Exit Slip How many moles are in 4. 5 x 1024 atoms of Ni? How many atoms are 78. 94 moles of iodine?

HOMEWORK!!!!! Page 86 Practice Problems 1 -3. Write the questions and show your work.

Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221. Math. 1 Objective: The learner will convert two step molar conversions. The learner will calculate the molecular weight of a compound, and apply it to molar conversions.

Entrance Slip Find the mass in grams of 3. 012 x 1024 atoms of Ca. The molar mass is 40. 08 g/mol

Converting Grams to atoms Example: 1. Calculate the number of atoms in a 356 g sample of Ti? 2. Determine the number of atoms in 7. 60 g of He. 3. 841 g Mn = _____ atoms of Mn

Converting Atoms to Grams Example: 1. Find the mass in grams of 2. 44 x 1024 atoms of carbon, whose molar mass is 12. 01 g/mol. 2. Find the mass in grams of 2. 11 x 1024 atoms of copper, whose molar mass is 63. 55 g/mol. 3. 5. 46 x 1024 atoms Pb = _____g Pb

Mole Relay Race Student #1 - Read the problem and set the problem up for the correct number of steps. Student #2 - Place the units in the set up. Student #3 - Fill in the correct conversion factors. Student #4 - Solve and write the answer with the correct number of sig. figs.

Exit Slip 4. 06 x 1024 atoms Cu = _______ g Cu 702 grams P = ____ atoms P

Molar Conversion 2 - Step Homework 1. Determine the number of moles of fluorine in 9. 23 x 10 -9 g of fluorine. 2. How many atoms of germanium are in 3. 00 x 106 g Ge? 3. What is the mass in grams of 1. 2 x 1025 atoms of the element bromine, Br? 4. How many atoms of beryllium are in 1. 67 x 103 g of Be? 5. What is the mass in grams of 9. 70 x 1023 atoms of magnesium, Mg?

Molecular Weight

What is the molecular weight of HCl?

Molecular weight – the mass in grams of one moles of a substance. (g/mol) What is the molecular weight of the following: Na. Cl H 2 O Ca(NO 3)2 Mg(NO 3)2

How many moles are in 67. 68 grams of Al 2 S 3?

345. 0 grams of Na. OH= ____ mol of Na. OH 5. 6 moles of HBr= _______ grams of HBr 200. 5 grams of Mg. Cl 2 = _______ mol of Mg. Cl 2

4. 5 moles Si. Cl 4 = _____ molecules Si. Cl 4 2. 3 moles of Ca. S = _______ formula units Ca. S Determine the number of moles of F 2 in 5. 6 x 1023 molecules of F 2.

Exit Slip How many grams are in 8. 9 moles of Li 2 O? How many molecules are in 5. 90 moles of CO?

267 grams of Li. Br = ______ formula units Li. Br 7. 8 x 1024 molecules of CO 2 = _____ grams of CO 2 149. 0 grams of OF 2 = ______ molecules OF 2

HOMEWORK Determine the mass in grams of 89. 0 moles of Na. NO 3? 6. 00 grams of B 2(SO 4)3= ____ formula units of B 2(SO 4)3 7. 8 x 1024 formula units of Ba 3 P 2 = ____ moles of Ba 3 P 2 5. 6 x 1025 formula units V 3(PO 4)5= _____ grams V 3(PO 4)5

Standard: Convert among the following quantities of a substance: mass, number of moles, and number of particles. Objective: The learner will review molar conversions.

Fine the molecular weight of potassium chlorate.

What is the mass in grams of 2. 50 moles of oxygen, O 2?

Ibuprofen, C 13 H 18 O 2, is the active ingredient in many nonprescription pain relievers. Its molar mass is 206. 31 g/mol. a. If the tablets in a bottle contain a total of 33 grams of ibuprofen, how many moles of ibuprofen are in the bottle? b. How many molecules are in the bottle? c. What is the total mass of carbon in 33 grams of ibuprofen?

How many moles are there in 6. 60 grams of (NH 4)2 SO 4? How many grams of nitrogen is in 6. 60 grams of ammonium sulfate? How many grams of oxygen are in 6. 60 grams of ammonium sulfate?

Practice Problems How many grams of Al are in 43. 8 g of Al 2 S 3? How many grams of chlorine are there in 0. 35 moles of CH 2 Cl 2? What is the mass of chlorine in 3. 36 grams of Mg. Cl 2? What is the mass of phosphorus in 135. 0 grams of K 3 PO 4? How many grams of nitrogen are in 2. 01 moles of N 2 O 5?

Let’s RACE

Mole Relay Race 1. Read the problem and set the problem up for the correct number of steps. 3. Place the units in the set up. 4. Fill in the correct conversion factors. 5. Solve and write the answer with the correct number of sig. figs.

Exit Slip How many grams of phosphorus are in 1. 02 moles of Ca 3(PO 4)2?

Homework How many grams of hydrogen are there in 4. 5 g of Ca(OH)2? How many grams of carbon are there in 3. 4 grams of C 12 H 22 O 11? How many grams of nitrogen are in 0. 35 moles of Cu(NO 3)2?

Standard: Analyze ionic and covalent compounds in terms of percent composition. Objective: The learner will evaluate the percentage composition of atoms in chemical formulas.

In what subjects would you most likely use percentages?

Percentage Composition

Percentage Composition What is percentage composition? the percent by mass of each element in a compound

Percentage Composition What is the equation for percentage composition? (Number of atoms of an element)(molar mass) X 100 = % of element Molecular weight of the compound in compound

Percentage Composition Example 1: Find the percentage composition of copper sulfide, Cu 2 S. Step 1: Write the equation. Step 2: Choose one element to solve. Step 3: Count the number of atoms that the element has. Substitute that number into the equation. Step 4: Find the molar mass of the element. Substitute that number into the equation. Step 5: Calculate the molecular weight of the compound. Substitute that number into the equation. Step 6: Solve Step 7: Check your work by adding the percentages. Your final answer should be at least 100%

Problem Calculate the percentage composition of the (NH 4)2 CO 3. Calculate the percentage composition of sodium nitrate, Na. NO 3. Calculate the percentage composition of calcium hydroxide, Ca(OH)2

Rally Coach

Group 1: Calculate the percentage composition of Ag 2 SO 4. Group 2: Calculate the percentage composition of Cu(NO 3)2. Group 3: Calculate the percentage composition of Na. Cl. Group 4: Calculate the percentage composition of Fe. SO 3. Group 5: Calculate the percentage composition of Ca. CO 3. Group 6: Calculate the percentage composition of H 2 S. Group 7: Calculate the percentage composition of Mg. F 2.

Student A: Calculate the percentage composition of Ag 2 SO 4. Student B: Calculate the percentage composition of Cu(NO 3)2.

Exit Slip Calculate the percentage composition of Al 2 S 3.

Classwork Write the statement. FIVE POINTS will be deducted is the statements are not written. TEN POINTS will be deducted if work is not shown. Calculate the percentage composition of Sr. Br 2. Calculate the percentage composition of Ca. SO 4. Calculate the percentage composition of Mg(CN)2. Calculate the percentage composition of Pb(NO 3)2. Calculate the percentage composition of Fe(Mn. O 4)3.

Standard: Convert percentage composition into an empirical formula. Objective: The learner will investigate empirical formulas.

Empirical Formula

Formulas and Percentage Composition Empirical formulas- a chemical formula that shows the composition of a compound. (ratios of atom)

Determine Empirical Formulas from Percentage Composition 1. Percent to mass (grams)-Assume that you have 100 g of the substance. 1. Mass (grams) to mole 1. Divide by the least number of moles. 1. Multiply 'til whole

Determine Empirical Formulas from Percentage Composition. Example 1. Chemical analysis of a liquid shows that it is 60. 0% C, 13. 4 %H, and 26. 6% O by mass. Calculate the empirical formula of this substance. 2. A dead alkaline battery is found to contain a compound of Mn and O. Its analysis gives 69. 6% Mn and 30. 4% O.

Determine Empirical Formulas from Percentage Composition. 1. A compound is 38. 77% Cl and 61. 23% O. 2. A liquid compound is 18. 0 % C, 2. 26% H, and 79. 7% Cl.

Determine Empirical Formulas from Percentage Composition Exit Slip. 1. A compound contains 5. 88% hydrogen and 94. 12% oxygen. What is the empirical formula?

Determine Empirical Formulas from Percentage Composition Homework. 1. A compound is made up of 92. 3% carbon and 7. 7% hydrogen. What is the empirical formula? 2. A compound contains 70. 0% iron and 30. 0% oxygen. What is the empirical formula?

Standard: Convert empirical formulas to molecular formulas. Objective: The learner will investigate molecular formulas.

Molecular Formula

Determine Molecular Formulas from Empirical Formula. Molecular formula- a chemical formula that shows the number and kinds of atoms in a molecule. Steps 1. Write the information that is given. 2. Find the molar mass of the empirical formula. 3. Solve using this formula. n= experimental molar mass of compound molar mass of empirical formula 4. Multiply the empirical formula by n to get the molecular formula.

Determine Molecular Formulas from Empirical Formula. Example: • The empirical formula for a compound is P 2 O 5. Its experimental molar mass is 284 g/mol. Determine the molecular formula of the compound. • Determine the molecular formula of a compound with an empirical formula of NH 2 and a molar mass of 32. 06 g/mol.

Determine Molecular Formulas from Empirical Formula. Example: • A sample with a formula mass of 34. 00 g/mol is found to consist of 0. 44 g H and 6. 92 g O. Find its molecular formula. • A compound with formula mass of 42. 08 g/mol is found to be 85. 64% carbon and 14. 36% hydrogen by mass. Find its molecular formula.

Determine Molecular Formulas from Empirical Formula. • A compound has an experimental molar mass of 78 g/mol. Its empirical formula is CH. What is its molecular formula? • A compound has the empirical formula CH 2 O. Its experimental molar mass is 90. 0 g/mol. What is its molecular formula? • If 4. 04 g of N combine with 11. 46 g O to produce a compound with a formula mass of 108. 0 g/mol, what is the molecular formula of this compound?

Determine Molecular Formulas from Empirical Formula. Exit Slip Determine the molecular formula of a compound with an empirical formula of C 2 H 4 S and a formula mass of 179 g/mol.