Download Honors Chemistry II Review 1. Express the following in scientific

Honors Chemistry II Review
1. Express the following in scientific notation:
a) 0.000000000 372m
b) 15,000,000,000m
2. Convert -78°C to Kelvin.
3. Gemstones are weighed in carats, with 1 carat = 200mg. What is the mass in grams of the Hope
Diamond, the world’s largest blue diamond at 44.4 carats?
4. For each of the following groups, determine the location, number of valence electrons, and charge of an
ion in that group:
(Alkali Metals, Halogens, Alkaline Earth Metals, Noble Gases, Nitrogen Group, and Oxygen Group)
5. How many significant figures are there in each of the following measurements?
a) 35.0445
d) 0.00450
b) 59.001
e) 67,000
c) 0.03003
f) 3.8200 x 103
6. Express the results of the following calculations with the correct number of significant figures:
a) 4.884 x 2.05
b) 94.61 / 3.7
c) 3.7 / 94.61
d) 5,502.3 + 24 + 0.01
e) 86.3 + 1.42 – 0.09
f) 5.7 x 2.31
7. Convert the following into SI units:
a) 5.4 inches
b) 66.31 lbs
c) 65mph
d) 98765.4 miles
8. Among many alternative units that be considered as a measure of time is the shake rather than the
second. Based on the expression, “faster than a shake of a lamb’s tail,” we’ll define 1 shake as equal to
2.5 x 10-4seconds. If a car is traveling at 55mph, what is its speed in cm/shake?
9. A small speck of carbon the size of a pinhead contains 1 x 1019atoms, and the circumference of the
earth at the equator is 40,075km. How many times around the earth would the carbon atom extend if they
were laid side by side? Hint… 1 atom = 1 x 10-10m
10. Copper metal has two naturally occurring isotopes: copper-63 (69.17%; atomic weight 62.94 amu) and
copper-65 (30.83; atomic weight 64.93 amu ). Calculate the atomic weight of copper and check your
answer to that on the periodic table.
11. Name the following compounds:
a) KBr
e) PbSO4
b) MnO2
f) NaNO3
c) CuS
g) PCl5
d) NO2
h) P4O6
12. Write the formula for the following compounds:
a) iron (III) sulfate
e) nitrogen trichloride
b) magnesium oxide
f) chromium (VI) phosphate
c) carbon tetrachloride
g) manganese (VII) phosphite
d) calcium hydroxide
h) cobalt (III) perchlorate
13. Write the name of the following acids:
a) H3PO3
d) HClO
b) HBr
e) H2SO4
c) HClO4
f) H2SO3
14. Write the formula for the following acids:
a) hydrochloric acid
d) nitric acid
b) perbromic acid
e) nitrous acid
c) bromous acid
f) hydrofluoric acid
15. A binary compound of zinc and sulfur contains 67.1% zinc by mass. What is the ratio of zinc and sulfur
atoms in the compound?
16. Naturally occurring boron consists of two isotopes, 10B (19.9%), with an atomic mass of 10.0129, and
11B (80.1%) with an atomic mass of 11.00931. What is the atomic weight of boron?
17. The commercial production of iron from iron ore involves a reaction of iron (III) oxide with carbon
monoxide to yield metallic iron and carbon dioxide. Write a balanced chemical equation and predict how
many moles of CO will react with 0.5 moles of iron (III) oxide.
18. Dichloromethane (CH2Cl2), a solvent used in the decaffeination of coffee beans, is prepared by the
reaction of methane (CH4) with chlorine. How many grams of dichloromethane result from the reaction of
1.85kg of methane if the yield is 43. 1%?
CH4 (g) + 2Cl2 (g)  CH2Cl2 (l) + 2HCl (g)
19. Lithium oxide is used aboard the space shuttle to remove water from the air supply according to the
equation:
Li2O (s) + H2O (g)  2LiOH (s)
Which reactant is limiting if there are 80kg of water to be removed and 65kg of Li2O available? How many
kg of the excess reactant remain?
20. After lithium hydroxide is produced aboard the space shuttle, it is used to remove exhaled carbon
dioxide from the air supply according to the following equation:
LiOH (s) + CO2 (g)  LiHCO3 (s)
How many grams of CO2 can 500g of LiOH absorb?
21. What volume of 0.250M H2SO4 is needed to react with 50mL of 0.100MNaOH (90, 3.19)? A balanced
equation is needed to begin this problem.
22. Ethyl alcohol contains carbon, hydrogen, and oxygen. On combustion analysis, 1.00g of ethyl alcohol
yields 1.174g of H2O and 1.910g of CO2. What is the empirical formula of ethyl alcohol?
23. Trioxane contains 6.71% H, 40.00% C and 53.28% O and has a molecular weight of 90.08g/mol.
Determine the molecular formula.
24. How many grams of each product result from the following reaction?
(2.65g BaCl2) + (6.78g H2SO4)  (x g BaSO4) + (y g HCl)
25. How many grams of cisplatin (Pt(NH3)2Cl2) are formed from 55.8g of K2PtCl4 and 35.6g of NH3 if the
reaction takes place in 95% yield based on the limiting reactant?
K2PtCl4 + 2NH3  2KCl + Pt(NH3)2Cl2
26. A graduated cylinder contains exactly 46.85mL of water. When an irregular piece of zinc, with a mass
of 8.261g, is placed in the graduated cylinder, the water rose to 53.90mL. What is the density of the zinc in
g/mL. Be sure to use significant figures in this problem.
27. What is the percent yield of ethyl acetate if 45.0g of acetic acid produces 46.0g of ethyl acetate?
C2H4O2 (l) + C2H6O (l)  C4H8O2 (l) + H2O (l)
Acetic Acid + Ethyl Alcohol  Ethyl Acetate + Water
28. In the previous reaction, 33.9g of ethyl alcohol reacts with excess acetic acid. How many grams of
water will be produced according to this reaction?