Download Section II - School District 27J

Section I
Time – 14 minutes
NO CALCULATORS MAY BE USED WITH THIS SECTION
Write the letter of the most correct answer on your answer sheet. Do not write on this test.
1.
Tungsten metal may be prepared by reducing WO3 with H2 gas. How many grams of tungsten may be
prepared from 0.0500 mol of WO3 with excess H2? (Water is also a product of this reaction.)
(A) 5.58 g
(B) 0.500 g
(C) 9.19 g
(D) 184 g
(E) 18.4 g
2.
___Fe(OH)2(s) + ___H3PO4(aq)  ____Fe3(PO4)2(s) + ____H2O (l)
When the equation above is balanced, the lowest whole-number coefficient for water is
(A) 3
(B) 1
(C) 9
(D) 6
(E) 12
3.
(A)
(B)
(C)
(D)
(E)
What is the oxidation state of chlorine in the compound potassium chlorate?
-1
+1
+3
+5
0
4.
A solution containing 0.20 mol of KBr and 0.20 mol of MgBr2 in 2.0 liters of water is provided. How
many moles of lead (II) nitrate must be added to precipitate all the bromide as insoluble PbBr2?
(A) 0.10 mol
(B) 0.50 mol
(C) 0.60 mol
(D) 0.30 mol
(E) 0.40 mol
5.
If 50.0 mL of 1.0 M AgNO3 is added to 50.0 mL of 0.50 M HCl, what is the concentration of silver ions
in the solution when the reaction reaches completion?
(A) 0.50 M
(B) 0.00 M
(C) 1.0 M
(D) 0.25 M
(E) 0.75 M
____C4H11N + ____O2  ____CO2 + ____H2O + ____N2
6.
When the equation above is balanced, the lowest whole number coefficient for O2 is
(A) 4
(B) 16
(C) 22
(D) 27
(E) 2
7.
A solution is prepared for qualitative analysis. The solution contains the following ions: Co 2+, Pb 2+ ,
3+
and Al . Which of the following will cause no observable reaction?
(A) Dilute NH3 is added
(B) Dilute K2CrO4 is added
(C) Dilute nitric acid is added
(D) Dilute K2S is added
(E) Dilute hydrochloric acid is added
8.
5 H2C2O4 + 2KMnO4 + 3 H2SO4  2MnSO4 + K2SO4 + 8H2O + 10CO2
How many moles of MnSO4 are produced when 1.0 mol of KMnO4, 5.0 mol of H2C2O4, and 3.0 mol of H2SO4
are mixed?
(A) 4.0 mol
(B) 5.0 mol
(C) 2.0 mol
(D) 2.5 mol
(E) 1.0 mol
9.
How many milliliters of 0.100 M sulfuric acid are required to neutralize 50.0 mL of 0.200 M potassium
hydroxide?
(A) 25.0 mL
(B) 30.0 mL
(C) 20.0 mL
(D) 50.0 mL
(E) 60.0 mL
10.
(A)
(B)
(C)
(D)
(E)
What should you do if you spill sulfuric acid on the countertop?
Neutralize the acid with HC2H3O2
Sprinkle solid NaOH on the spill
Neutralize the acid with NaHCO3
Neutralize the acid with MgSO4
Use paper towels to soak up the acid
Section II
Time – 30 minutes
Complete all portions of the four problems listed below. You must show all of your work to
receive credit. YOU MAY USE YOUR CALCULATOR FOR THIS PORTION. Do not
write on this test.
A sample of an unknown monoprotic acid was analyzed. The sample
contained 40.0 % carbon, 6.71 % hydrogen. The remainder of the sample was
oxygen.
a.
Determine the empirical formula of the acid.
b.
A 0.2720 g sample of the acid is titrated with standard sodium hydroxide
solution. Determine the molar mass of the acid if the sample required 45.00 mL of
0.1000 M sodium hydroxide to reach its endpoint.
c.
What is the molecular formula for this acid? (EC ~ NAME IT!)
1.
2.
Copper metal reacts with nitric acid to produce copper (II) nitrate, nitrogen
monoxide and water.
a.
Write the balanced chemical equation.
b.
Identify the oxidizing agent.
c.
If a 0.300 mol sample of copper reacts with 10.0 mL of 12.0 M nitric
acid, how many moles of nitrogen monoxide gas will form?
d.
If 0.672 g of nitrogen monoxide is recovered from this reaction,
calculate your percent error.
3.
Balance the following redox reaction that takes place in an acidic solution:
Co(OH)3 + Sn  Co(OH)2 + HSnO21-
4.
Calculate the chloride ion concentration in a solution prepared by dissolving
8.99 g of calcium chloride in enough water to prepare 150.0 mL of solution.