Download Topics on Chapter 10 Test: The Mole

Topics on Chapter 10 Test: The Mole
10.1 Measuring Matter
Mole
Mole conversions involving atoms and molecules
10.2 Mass and the Mole
Mole conversions involving grams in an element
10.3 Moles of Compounds
Molar mass
Mole conversions involving grams of a compound
Mole conversion involving liters of gas at STP
Mixed conversions
10.4 Empirical and Molecular formulas
Percent by mass calculations
Empirical formula calculations
Molecular formula calculations
10.5 Formulas of Hydrates
Hydrates
Problems from your textbook, pg 358-361
90, 92, 100, 109, 117, 131, 135, 136, 138, 142, 161, 162, 164, 167,
172, 173, 179
Review for Test on Chapter 10 – The Mole
1. Convert .669 moles of Au to atoms of Au
2. Convert 3.049 × 1024 atoms of Zn to mole of Zn
3. Convert 9.60 × 1022 molecules of H2CO3 to moles of H2CO3
4. Convert 3.667 moles of of magnesium nitrite to grams of magnesium nitrite
5. Convert 7.09 × 10-2 g of (NH4)2CO3 to moles of (NH4)2CO3
6. Convert 450 L of Ne gas to moles of Ne gas
7. Convert 2.91 × 10-3 mol of CO2 to liters of CO2 at STP
8. Convert 9.55 × 1022 atoms of Ar gas to L of Ar gas at STP
9. Convert 8.94 g of H2O to molecules of H2O
10. Convert 990 L of O3 at STP to grams of O3.
11. Determine the percent composition for Pb(NO3)2
12. Determine the percent composition for Aluminum sulfate
13. What is the empirical formula of C5H10O20
14. Determine the empirical formula for a compound with a % composition of 75% carbon and 25%
hydrogen
15. Determine the empirical formula for the compound with the % composition 32.4% sodium, 22.5
% sulfur, and 45.1 % oxygen.
16. Determine the empirical formula for the compound with the % composition 26.6 % K, 35.4 % Cr,
and 38.0 % O.
17. Determine the molecular formula for the compound with an empirical formula of C2H3O2 and a
molar mass of 119 g.
18. Determine the molecular formula for compound having the following analyses: 54.53 % carbon,
9.15 % hydrogen, 36.32 % oxygen; molar mass of molecular formula 88 g.
19. A 0.400 g sample of a white powder contains 0.141 g potassium, 0.115 g sulfur, and 0.144 g
oxygen. What is the empirical formula for the compound? (HINT: first find % composition)
20. Histamine is a substance that is released by cells in response to injury, infection, stings, and
material that cause allergic response, such as pollen. Histamine causes dilation of blood vessels
and swelling due to accumulation of fluid in the tissues. People sometimes take antihistamine drugs
to counteract the effects of histamine. A sample of histamine having a mass of 385 mg is
composed of 208 mg of carbon, 31 mg hydrogen, and 146 mg nitrogen. The molar mass of
histamine is 111g/mol. What is the molecular formula for histamine?
#TBTs!!!
1.
What is the difference between the independent and dependent variable?
2.
How many significant figures does a number have? (example: .00670)
3.
Calculations with correct significant figures (example: 2.65 x .035)
4.
Converting one metric unit to another metric unit (keeping in mind significant figures - example:
350.0 mL to L)
5.
Is a change a chemical or physical change? (example: snow melting, iron rusting, ...)
6.
Percent by mass problems (example: what is the percent of oxygen in a compound that
contains 12.6 g of oxygen and 46.3 g of nitrogen, and 5.67 g of hydrogen.
7.
Number of neutrons, protons, and electrons mass number and atomic number. (example:
How many p+, n, and e- does the atom 4019K have?)
8.
Writing nuclear equations (example: what is the equation for the alpha decay of curium-249)
9.
Writing electron configurations(example: Mg 1s2, 2s2, 2p6, 3s2)
10.
Writing orbital diagrams (example: ↑↓
11.
Groups of the periodic table (example: what group does silver belong to?)
12.
Stating the number of valence electrons (example: how many valence electrons does silicon
have?)
13.
Writing the name for ionic compounds (example: Pb(NO3)2)
14.
Writing the formula for ionic compounds (example: Iron (II) hydroxide)
15.
What is the Lewis dot structure for a molecule (example: NH3)
16.
Is a molecule polar or nonpolar (example: NH3)
17.
What type of reaction is listed (example: CaO (s) + CO2 (g) → CaCO3 (s))
18.
Balance a chemical equation (example: silver nitrate (aq) + sodium sulfide (aq) → silver sulfide
(s) + sodium nitrate (aq))
↑↓
1s
↑↓ ↑↓ ↑↓
2s
↑↓ )
2p
3s