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