Post on 16-Jan-2016
The MoleAA. Review
Must turn in your packet with notes stapled to it before you
can take the test
Define (*and how to calculate)
1. Molar Mass*
2. 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) 3. Empirical Formula*
4. 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)5. Percent Composition*
6. 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:
a. Oxygen
b. 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:
a. 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: 21.6% 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