The Mole AA. Review Must turn in your packet with notes stapled to it before you can take the test.

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Presentation transcript:

The Mole AA. Review Must turn in your packet with notes stapled to it before you can take the test

Define (*and how to calculate) Molar Mass* Mole* Mass in grams of 1 mole of any pure substance. Add individual masses from PT SI base unit used to measure amount of substance Use conversion ratios btw molar mass and representative particles

Define (*and how to calculate) Empirical Formula* Molecular Formula* Formula that shows lowest, whole # mole ratio Find moles, divide by smallest, multiple ‘til whole number ratios - Formula that shows all atoms in a molecule - Divide MF mass by EF mass, multiply EF by the whole number answer.

Define (*and how to calculate) Percent Composition* Representative Particles (are they atoms, molecules, or formula units?)* - Percent by mass of each element in a compound. - Find molar mass, divide individual masses by molar mass, times by 100. Element = atoms Covalent Compound = molecule Ionic Compound = formula unit * Convert with Avogador’s #

Define (*and how to calculate) 7. Avogadro’s Number # of representative particles in a mole 1 mole = 6.02 x 1023

8. Determine the molar mass of the following: Oxygen Nitrogen dioxide c. NH4NO3 O2 = 2 (16.00) = 32.00 g/mol NO2 = 1(14.01) + 2(16.00) = 46.01 g/mol NH4NO3 = 1(14.01) + 4(1.01) + 1(14.01) + 3(16.00) = 80.06 g/mol

9. Convert the following: a. 4.53 moles of carbon monoxide to grams

9. Convert the following: b. 0.67 g of chlorine gas (Cl2) to moles

9. Convert the following: c. 2.41  1024 molecules of (NH4)SO3 to moles

10. Convert the following: 20.6 moles of SO2 to grams

10. Convert the following: b. 4.44 g of iron (II) oxide to molecules

10. Convert the following: c. 8.322 x 1024 molecules of N2 to moles

11. Determine the percent composition of CuSO4

12. Determine the empirical formula of a sample that has: 21 12. Determine the empirical formula of a sample that has: 21.6% sodium (Na), 33.3% chlorine (Cl), and 45.1% oxygen (O)

13. Determine the molecular formula of the following compound: Nitrogen = 30.4%, Oxygen=69.6%. Molecular weight = 92 g/mol