Measuring matter The mole

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Presentation transcript:

Measuring matter The mole Ch. 10 Section 1 Measuring matter The mole Ch. 10 NOTES

How do you measure matter? By mass By volume By counting: specific units Pair Dozen Baker’s dozen Ch. 10 NOTES

Mole “mol” Counting unit used for atoms Italian scientist Amedeo Avogadro di Quaregna (1776–1856) who helped clarify the difference between atoms and molecules. Ch. 10 NOTES

Mole 6.02x1023 particles = 1 mole 1 mole contains Avogadro’s number of particles (6.02 × 1023) Ch. 10 NOTES

Particles – moles conversion A) Obtain the number of sucrose molecules contained in 3.50 mol of sucrose. Ch. 10 NOTES

Particles – moles conversion B) How many particles of zinc are contained in 2.50 mol of zinc? Ch. 10 NOTES

Particles – moles conversion C) How many particles of silver nitrate are there in 3.25 of silver nitrate? Ch. 10 NOTES

Particles – moles conversion D) How many moles of aluminum are equivalent to 5.75x1024 atoms of aluminum? Ch. 10 NOTES

Particles – moles conversion E) There are 2.50x1020 atoms of iron. How many moles are equivalent to this amount? Ch. 10 NOTES

Chapter 10 Section 2 and 3 Mass of a mole Ch. 10 NOTES

Molar mass Mass of 6.02x1023 particles average atomic mass or molar mass Ionic compounds: “formula weight” Covalent compounds: “molecular weight” Ch. 10 NOTES

Molar mass of an element C Mg Fe 12.01 g/mol 24.31 g/mol 58.85 g/mol Ch. 10 NOTES

How is the molar mass of a compound determined? Add together atomic mass of all atoms in compound Ch. 10 NOTES

Molar mass of NaCl 1 Na x 22.99 g/mol 1 Cl x 35.5 g/mol 23.0 g/mol Ch. 10 NOTES

Molar mass of water H2O Add atomic masses 2 H x 1.01 g/mol 1 O x 16.0 g/mol 2.02 g/mol + 16.0 g/mol 18.02 g/mol Ch. 10 NOTES

Molar mass of sugar C6H12O6 Add atomic masses 6 C x 12.01 g/mol 12 H x 1.01 g/mol 6 O x 16.0 g/mol 72.06 g/mol 12.12 g/mol + 96.0 g/mol 180.18 g/mol Ch. 10 NOTES

Moles-Mass conversion A) What is the mass in grams of 3.00 mol of NaCl? Ch. 10 NOTES

Moles-Mass conversion B) What is the mass of 9.45 mol of aluminum oxide (Al2O3)? Ch. 10 NOTES

Moles-Mass conversion C) Calculate the mass in grams of 2.50 mol of Fe(OH)2 Ch. 10 NOTES

Moles-Mass conversion D) How many moles are contained in 92.2 g of iron (III) oxide? (Fe2O3) Ch. 10 NOTES

Moles-Mass conversion E) How many moles are contained in 100.0 g of calcium chloride? (CaCl2) Ch. 10 NOTES

Empirical and Molecular formulas Ch. 10 Section 4 Empirical and Molecular formulas Ch. 10 NOTES

Ch. 10 Section 5 Hydrates Ch. 10 NOTES

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