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1) Atoms surrounded by eight valence electrons tend to lose electrons.
2) At constant temperature, reducing the volume of a gaseous equilibrium mixture
causes the reaction to shift in the direction that increases the number of moles of gas in
the system.
3) The energy produced by the sun is the result of nuclear fusion.
4) The effusion rate of a gas is proportional to the square root of its molar mass.
5) The melting of a substance at its melting point is an isothermal process.
6) Changes in the coordination sphere of a complex compound may lead to changes in
________.
A) color
B) physical properties
C) chemical properties
D) stability
E) all of the above
7) Calculate the molarity of phosphoric acid (H3PO4) in a 38.4% (by mass) aqueous
solution.
A) 0.115 m
B) 0.206 m
C) 0.0514 m
D) 0.103 m
E) The density of the solution is needed to solve the problem.
8) A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH
solution. The equivalence point is reached with 62.5 mL of the base. The concentration
of H2SO4 is ________ M.
A) 0.234
B) 0.469
C) 0.150
D) 0.300
E) 0.938
9) The hybridization of carbon in the H€C N: molecule is ________.
A) sp2
B) s2p
C) s3p
D) sp
E) sp3
10) Which reaction produces an increase in the entropy of the system?
A) Ag+ (aq) + Cl- (aq) --> AgCl (s)
B) CO2 (s) --> CO2 (g)
C) H2 (g) + Cl2 (g) --> 2 HCl (g)
D) N2 (g) + 3 H2 (g) --> 2 NH3 (g)
E) H2O (l) --> H2O (s)
11) Which energy difference in the energy profile below corresponds to the activation
energy for the forward reaction?
A) x
B) y
C) x + y
D) x - y
E) y - x
12) Given the data in the table below, ΔH° for the reaction
2CO (g) + O2 (g) → 2CO2 (g)
is ________ kJ.
A) -566.4
B) -283.2
C) 283.2
D) -677.0
E) The ΔH°f of O2 (g) is needed for the calculation.
13) The energy of a photon that has a frequency of 1.821 X 1016 s-1 is ________ J.
A) 5.44 X 10-18
B) 1.99 X 10-25
C) 3.49 X 10-48
D) 1.21 X 10-17
E) 5.46 X 10-24
14) Given the data in the table below, ΔH°rxn for the reaction
4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l)
is ________ kJ.
A) -1172
B) -150
C) -1540
D) -1892
E) The ΔH°f of O2 (g) is needed for the calculation.
15) A buffer solution with a pH of 4.40 is prepared with 0.78 M Na C2H3O2 and
________ M HC2H3O2.The Ka of HC2H3O2 is 1.8 x 10-5.
A) 1.7
B) 3.5
C) 4.1 x 104
D) 0.35
E) 0.86
16) A gas at a pressure of 325 torr exerts a force of ________ N on an area of 5.5 m2.
A) 1.8 x 103
B) 59
C) 2.4 x 105
D) 0.018
E) 2.4
17) Which of the following is most likely to exhibit liquid-crystalline behavior?
A) CH3CH2-C(CH3)2-CH2CH3
B) CH3CH2CH2CH2CH2CH2CH2CH3
C) CH3CH2CH2CH2CH2
-
D)
E)
18) The reaction A --> B is first order in [A]. Consider the following data.
The half-life of this reaction is ________ s.
A) 5.0
B) 0.97
C) 7.1
D) 3.0
E) 0.14
19) Which one of the following is not true concerning 2.00 L of 0.100 M solution of
Ca3(PO4)2?
A) This solution contains 0.200 mol of Ca3(PO4)2.
B) This solution contains 0.800 mol of oxygen atoms.
C) 1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions.
D) There are 6.02 x 1022 phosphorus atoms in 500.0 mL of this solution.
E) This solution contains 0.600 mol of Ca2+.
20) Elements in Group 2A are known as the ________.
A) alkaline earth metals
B) alkali metals
C) chalcogens
D) halogens
E) noble gases
21) The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s)
and ________ bonded electron pair(s) in its valence shell.
A) 1, 4
B) 2, 4
C) 4, 0
D) 4, 1
E) 4, 2
22) The acid and salts of which halogen-oxyanion are the most stable?
23) To produce maximum heat, an explosive compound should have ________
chemical bonds and decompose to molecule with ________ bonds.
24) Hydrogenation of what alkyne produces propane?
25) Calculate the bond energy of C€F given that the heat of atomization of CHFClBr is
1502 kJ/mol, and that the bond energies of C€H, C€Br, and C€Cl are 413, 276, and 328
kJ/mol, respectively.
26) The world's largest desalinization plant is in ________ and uses the process of
________ to produce drinking water.
27) The relationship of absorbed light to the concentration of the substance absorbing
the light is governed by ________.
28) Water can be formed from the stoichiometric reaction of hydrogen with oxygen:
2H2 (g) + O2 (g) → 2H2O (g)
A complete reaction of 5.0 g of O2 with excess hydrogen produces ________ g of H2O.
29) What is the oxidation state of the iron atom in CaNa[Fe(CN)6]?
30) When living tissue is irradiated most of the energy is absorbed by ________.
