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Chapter 9 2pt each
1. The number of valence electrons in the element Nitrogen is
a. 2
b. 3
c. 5
d. 7
2. As bond length _________ the bond strength is __________.
a. lengthens/weaker
c. shortens/stronger
b.shortens/weaker
d. lengthens/stronger
3. In which molecule is the carbon/oxygen bond the strongest? (CO, CO2,CO3-2,
H2CO3)
a. CO
c. CO3-2
b. CO2
d. H2CO3
4. The formula for sulfurous acid is.
a. SF2
b. H2SO4
c. HSO3
d. HSF
5. Which of the following bonds is most negatively charged?
a. C-H
b. C-S
c.C-N
d. C-O
6. Based on symmetry which one of these molecules is non-polar?
a. H3O+
b. PCl5
c. H2O
d. NH3
7. The molecular shape of PH3 would be.
a. Trigonal bipyramidal
b. Bent
c. Linear
d. Trigonal pyramidal
8. As I move from left to right the electronegativity ____________and as I move
from top to bottom it ___________.
a. Increases/Decreases
b. Decreases/Increases
c. stays the same/Increases c. Decreases/stays the same
9. What is the correct name for this compound? NO
a. Nitrous oxide
b. Nitric acid
c. Nitrogen monoxide
d. Mononitrogen monoxide
10. Draw the Lewis structures for each of the following molecules or ions. 2pt each
a. H2S
b. SO2
c. PO3-3
Final Exam Ch 10, 11, 12, 22, 16
Chapter 10 2pts each
1. The products of a combustion reaction are always:
a. carbon dioxide and water b. oxygen and water
c. carbon dioxide and oxygen
d. none of these
2. The solvent in an aqueous solution is always
a. Oxygen
b. an acid
c. a base
d. water
3. A solid produced during a chemical reaction is called a (an)
a. solute
b. precipitate
c. spectator ion
d. solvent
4. Balance the following equation.
Fe(s) + H2O(l)  Fe2O3(s) + H2(g)
5. Balance the following equation
NH3(aq) + O2(g)  NO(g) + H2O(l)
6. The equation in #14 is an example of
a. Decomposition rxn
b. Single replacement rxn
c. Double replacement
d. Combustion rxn
7. In a double replacement reaction the ______reacts with the (an) ______ to
form______________.
a. Anion/Cation/ single product
b. Cation/Anion/Two different
compounds
b. Metal/Oxygen/Two different compounds d. Element/Element/Water
8. What is the difference between the net ionic equation and the ionic equation?
2pts
9. Please write the word equation for the following reaction.
CaCO3(s) + 2HCl(aq)  CaCl2(aq) + H2O(l) + CO2(g)
Chapter 11
10. Determine the number of moles of 84.6 L of tetrahydrogen nonoxide.2pt
11. Find the mass in grams of 5.00 x 1023 molecules of fluorine gas.2pt
12. How many representative particles are in each of these substances? 6pts
a. Cl2
b. AlCl3
c. Kr
13. How many nitrogen atoms are in 10 moles of nitrogen dioxide? 2pt
14. How many kilograms of calcium can be recovered from 550 Kg of the
compound calcium carbonate? 3pt
15. The Percent composition of a compound is 24%C and 76% F. What is the
empirical formula? If the molecular mass is 150 grams, what is the molecular
formula? 6pt
16. What is the formula and name of a hydrate that is 85.3% Barium and 14.7%
water? 4pt
27. Why is the difference between the atomic mass and the molar mass? 2pts
17. Extra credit: the number 6.02 x 1023 is also called ____________ number.
Chapter 12: Multiple Choice: Write the letter of the best answer in
the blank to the left of the question. 2pts each
____28. The substance that limits or determines the amount of
product that can be formed in a reaction is called
__________________.
a. limiting reagent
b. excess reagent
c. actual yield
d. theoretical yield
____29. The amount of product that forms when a reaction is carried
out in the laboratory is called a ___________________.
a. limiting reagent
b. excess reagent
c. actual yield
d. theoretical yield
____30. In a chemical reaction
a. mass is conserved
c. moles are conserved
conserved
b. atoms are conserved
d. both mass and atoms are
Perform these calculations showing ALL you work for extra credit!
31. Ammonia, NH3 is a typical ingredient in household cleaners. It is
produced through a combination reaction involving nitrogen gas and
hydrogen gas. If 10 moles of hydrogen gas reacts with an excess of
nitrogen gas, how many moles of ammonia are produced? 2pts
N2(g) + 3H2(g)  2NH3(g)
32. How many grams of CO are needed to react with an excess of
Fe2O3 to produce 558 g of Fe? The equation for the reaction is: (2pts)
Fe2O3(s) + 3CO(g)  CO2(g) + 2Fe(s)
33. What is the limiting reagent when 50 g of nitrogen reacts with
10.7 g of hydrogen according to this balanced equation? (4pts)
N2(g) + 3H2(g)  2 NH3(g)
34. (a) if 4 g of hydrogen gas are made to react with excess carbon
monoxide, how many grams of CH3OH can theoretically be
produced according to the following equation? (2pts)
CO(g) + 2H2(g)  CH3OH(l)
(b) If 28 g of CH3OH are actually produced, what is the percent
yield? (2pts)
Chapter 16
35. The specific heat of ethanol is 2.44 J/gxC. How many kilojoules of
energy are required to heat 50g of ethanol from -20.0 degrees C to
68.0 degrees C? 3pts
a. 10.7 kJ
b. 2.44 kJ
c. 8.30 kJ
d. 1.22 kJ
36. 3.00 g of aluminum foil is placed in an oven and heated from 20.0
degrees C to 662.0 degrees C. If it absorbs 1728 J of heat, what is the
specific heat of aluminum? 3pts
a. 0.131 J/gxC
b. 0.897 J/gxC
c. 0.870 J/gxC
d. 2.61 J/gxC
37. A 15.6g sample of ethanol absorbs 868 J as it is heated. If the
initial temperature of ethanol was 21.5 degrees C and the specific
heat of ethanol is 2.44 J/gxC, then what is the final temperature of
the ethanol? 3pts
a. 44.3 C
b. – 44.3 C
c. 22.15 C
d. 88.6 C
38. Determine the delta H for the reaction of aluminum and sulfur
dioxide.
4Al(s) + 3SO2(g)  2Al2O3(s) + 3S(s)
Use the following equations.
4Al(s) + 3O2(g)  2Al2O3(s) Delta H = -3352 kJ/mole
S(s) + O2(g)  SO2(g)
Delta H = -297 kJ/mole
a. -4243 kJ
c. -3649 kJ
b. -3055 kJ
d. -2461 kJ
39. In describing a chemical reaction, what is meant by the system? The
surroundings? 3pts
40. Describe the differences between enthalpy, entropy, and free energy
and give the correct symbols for each concept. 6pts
Chapter 22
41. Write the structural formulas for each of the following.4pts
a. 2-methyhexane
b. 2,3-dimethypentane
42. Name the compound represented by each of the following
structural formulas. 4pts
a. CH3CH2CH2CH2CH3
c. CH3CH2CHCH2CH3
|
CH2
|
CH3
43. Write the name and draw the structure of the alkyl group that
corresponds with the following alkanes. 6pts
a. methane
b. butane
c. octane
44. Explain the difference between a saturated hydrocarbon and an
unsaturated hydrocarbon chain. 2pts
45. Extra Credit: Name one thing you liked or enjoyed learning
about and one thing you did not like learning about this class. 2pts