Uploaded by Nicole Thorson

Revision Multiple Choice

1. Which pair of substances could be separated by
mixing with water and filtering?
(A) NaNO3 and K2SO4 (B) CH3OH and CH3COCH3
(C) MgCO3 and Fe(OH)3
(D) KCl and CuS
2. Which gas produces an acidic solution when bubbled
into water?
(A) NH3
(B) Cl2
(C) H2
(D) CH4
3. A dilute HCl solution is to be prepared from a more
concentrated solution. Which of pieces of glassware will
give the highest level of precision?
(A) graduated cylinder and volumetric flask
(B) two graduated cylinders
(C) pipet and graduated cylinder
(D) pipet and volumetric flask
1) 2Mn2+(aq) + 4OH¯(aq) + O2(g) ---> 2MnO2(s) +
2) MnO2(s) + 2I¯(aq) + 4H+(aq) ---> Mn2+(aq) + I2(aq) +
3) 2S2O32¯(aq) + I2(aq) ---> S4O62¯(aq) + 2I¯(aq)
(A) 0.5
(B) 1
(C) 2
(B) 0.60 M
(C) 0.35 M (D) 0.30 M
12. How many electrons are present in 2.0 x 10¯3 moles
of 188O2¯?
(A) 1.2 x 1021
(C) 1.2 x 1022
(B) NaOH
(D) SiO2
(D) 4
11. A 15 mL sample of 0.20 M MgCl2 is added to 45 mL
of 0.40 M AlCl3. What is the molarity of Cl¯ ions in the
final solution?
(A) 1.0 M
4. Which substance is likely to show the greatest change
in mass when exposed to air?
(A) Al
(C) CaCO3
10. These three equations describe an oxidationreduction method for determining dissolved oxygen in
water. How many moles of S2O32¯ are equivalent of each
mole of O2?
(B) 9.6 x 1021
(D) 1.9 x 1022
13. In which change of state are covalent bonds broken?
5. Which is a yellow solid?
(A) C
(B) Na
(C) S8
(D) I2
6. An alloy of gold and silver contains 38.5% silver by
mass and has a density of 14.6 g mL¯1. What is the
molar concentration of silver in this alloy?
(A) 52.1 mol L¯1
(C) 3.57 mol L¯1
(B) 45.6 mol L¯1
(D) 2.64 mol L¯1
(A) evaporation of water
(B) fusion of sodium chloride
(C) vaporization of diamond
(D) sublimation of dry ice
14. By what factor does the average velocity of a
gaseous molecule increase when the absolute
temperature is doubled?
(A) 1.4
7. As2S3 reacts with O2 to give SO2 and As2O3. What is
the smallest whole number coefficient for O2 when the
equation for this reaction is balanced correctly?
_As2S3(s) + _O2(g) ---> _As2O3(s) + _SO2(g)
(A) 3
(B) 5
(C) 7
(D) 9
8. A 0.242 g sample of potassium is heated in oxygen.
The result is 0.440 g of a crystalline compound. What is
the formula of this compound?
(A) KO (B) K2O
(C) KO2
(D) KO3
9. What volume of 3.0 M Na2SO4 must be added to 25
mL of 1.0 M BaCl2 to produce 5.0 g of BaSO4?
(A) 7.2mL
(B) 8.3mL
(C) 10.0mL (D) 14mL
(B) 2.0
(C) 2.8
(D) 4.0
15. Which species is expected to have the highest boiling
point at 1 am pressure?
(A) O2
(B) CO
(C) CO2
16. Which combination of vapor pressure,
intermolecular forces and ΔHvaporization is matched
(A) high
(B) high
(C) low
(D) low
17. Which halogen in its standard state has the greatest
absolute entropy per mole?
(A) F2(g)
(B) Cl2(g)
(C) Br2(l)
(D) I2(s)
18. Calculate ΔH° for this reaction.
C2H2(g) + 2H2(g) ---> C2H6(g)
ΔHcombustion, kJ mol¯1
(A) -312 kJ
(B) -26 kJ
(C) +26 kJ
(D) +312 kJ
24. The reaction between KMnO4 and H2C2O4 can be
followed by monitoring the disappearance of the purple
color of the MnO4¯ ion. These data were obtained for the
reaction carried out at a constant temperature of 25 °C.
Initial Rate,
Exp [MnO4¯]
[H2C2O4] Disappearance
of MnO4¯ (aq), M s¯1
1 1.08 x 10¯2 M 1.98 M 5.4 x 10¯5
1.08 x 10¯2 M 3.97 M
1.1 x 10¯4
2.17 x 10¯2 M 1.98 M
2.1 x 10¯4
Specify the order of this reaction with respect to [MnO4¯]
and [H2C2O4]
[MnO4¯] [H2C2O4]
(A) 1st order 2nd order
19. For which process would ΔS° be expected to have
the greatest positive value?
(B) 2nd order 1st order
(C) 1st order 1st order
(A) O2(g) + 2H2(g) ---> 2H2O(g) (B) H2O(s) ---> H2O(l)
(C) H2(g) + I2(g) ---> 2HI(g) (D) N2O4(g) ---> 2NO2(g)
25. For which reaction order is the half-life independent
of the initial concentration?
20. (1/2) N2(g)+ (3/2) H2(g) ---> NH3(g)
For this reaction at 25 °C, ΔG°f is -16.5 kJ mol¯1. What
is the equilibrium constant, Keq, for this reaction at this
(A) 1.08 (B) 7.80 x 10 (C) 4.57 x 10
(D) 2nd order 2nd order
(D) 2.98 x 10
21. What are the signs for ΔH, ΔS, and ΔG for the
freezing of liquid water at -10 °C?
(A) I only
(C) both I and II
II second order
(B) II only
(D) neither I nor II
26. What is the activation energy for the reverse of this
N2O4(g) ---> 2NO2(g)
Data for the given reaction is: ΔH = + 54.0 kJ and Ea =
+57.2 kJ.
(A) +
(B) -
(C) -
+ -
(A) -54.0 kJ (B) +3.2 kJ (C) +60.2 kJ (D) +111.2 kJ
(D) -
22. Which of these factors affect the value of the specific
rate constant for the reaction 2A(g) ---> B(g)?
27. How does an increase in temperature affect the rates
of the foward and reverse reactions for an exothermic
rate of foward reaction rate of reverse reaction
I concentration
remains the same
(A) I, II, and III
(C) II and III only
I first order
II pressure
III temperature
(B) I and II only
(D) III only
23. Which statement about work and heat is true?
(A) A given quantity of heat can be completely
converted to work.
(B) Heat and work are both state functions.
(C) Some heat is always produced when work is done.
(D) Work is a state function, whereas heat is not.
28. The reaction between chloroform, CHCl3(g), and
chlorine, Cl2(g), to form CCl4(g) and HCl(g) is believed
to occur by this series of steps.
Step 1 Cl2 ---> Cl(g) + Cl(g)
Step 2 CHCl3(g) + Cl(g) ---> CCl3(g) + HCl(g)
Step 3 CCl3(g) + Cl(g) ---> CCl4(g)
If this reaction is first order in CHCl3 and half order in
Cl2, which statement about the relative rates of step 1, 2,
and 3 is correct?
(A) Step 1 is the slowest.
(B) Steps 1 and 2 must both be slow.
(C) Step 2 must be slower than step 1.
(D) Step 3 must be the slowest
34. Which mixture forms a buffer when dissolved in 1.0
L of water?
(A) 0.2 mol NaOH + 0.2 mol HBr
(B) 0.2 mol NaCl + 0.3 mol HCl
(C) 0.4 mol HNO2 + 0.2 mol NaOH
(D) 0.5 mol NH3 + 0.5 mol HCl
29. This reaction occurs readily above 500 °C.
2HgO(s) ---> 2Hg(l) + O2(g)
What is the equilibrium for this reaction?
35. The equilibrium constant for this reaction is 3.6 x
OCl¯(aq) + H2O(l) <===> HOCl(aq) + OH¯(aq)
What is Ka for HOCl?
(A) K = [Hg]2[O2] / [HgO]2
(B) K = [Hg][O2] / [HgO]
(C) K = [Hg]2[O2]
(D) K = [O2]
(A) 2.8 x 10¯8
(B) 3.6 x 10¯7
(C) 6.0 x 10¯4
(D) 2.8 x 106
30. Consider this equilibrium, for which ΔH < 0.
HgO(s) + 4I¯(aq) + H2O(l) <===> HgI42¯ + 2OH¯
Which changes will increase the equilbrium
concentration of HgI42¯?
36. For which titration would the use of phenophthalein
introduce a significant error?
Kindicator for phenolphthalein = 1 x 10¯9
I Increasing the mass of HgO(s) present
II Increasing [I¯]
III Adding 1 M HCI
(A) I only
(B) II only
(C) II and III only
(D) I, II, and III
31. The equilibrium constant for this reaction is
approximately 10¯3.
HPO42¯(aq) + HCO3¯(aq) <==> H2PO4¯(aq) + CO32¯(aq)
Which is the strongest conjugate base in this reaction?
(A) HPO42¯(aq)
(B) HCO3¯(aq)
(C) H2PO4¯(aq)
(D) CO32¯(aq)
(A) 2.2 x 10¯9
(C) 1.8 x 10¯8
32. A weak acid, HX, has Ka = 9.0 x 10¯6. Within which
range does the percent dissociation for a 0.01 M HX
solution lie?
(A) between 1.0% and 10% (B) between 0.10% and 1.0%
(C) between 0.01% and 0.10%
(D) less than 0.01%
33. Which salt dissolves in water to produce a solution
with a pH < 7?
(A) NaC2H3O2
(C) AlCl3
37. When solid lead iodide is added to water, the
equilibrium concentration of I¯ becomes 2.6 x 10¯3 M.
What is the Ksp for PbI2?
(B) Ba(NO3)2
(D) KClO4
(B) 8.8 x10¯9
(D) 3.5 x 10¯8
38. When these standard half reactions are combined to
give a spontaneous reaction in a voltaic cell, what is the
cell voltage?
Standard Reduction Potentials,
Sn (aq) + 2e¯ ---> Sn(s)
-0.14 V
Ag (aq) + e¯ ---> Ag(s)
+0.80 V
(A) 1.74 V
(C) 0.94 V
(B) 1.46 V
(D) 0.66 V
39. How many moles of elections are transferred when
this equation is balanced with the smallest whole number
_IO3¯ + _H2O2 + _H+ ---> _I2 + _O2 + _H2O
(A) 2
(B) 4
(C) 5
(D) 10
40. When anions undergo oxidation, they move toward
A. anode of a voltaic cell and the cathode of an
electrolytic cell
B. cathode of a voltaic cell and the anode of an
electrolytic cell
C. anodes of both types of cells
D. cathodes of both types of cells
B. N < C < Si
D. Si < N < C
1.31 3.39
5.30 7.47
46. In the Lewis structure for the BrF4¯ ion, how many
lone pairs of electrons are placed around the central atom?
(B) 1
(C) 2
(D) 3
47. What term is used for the measure of an atom's
attraction for the electrons that constitute a covalent
42. These are the first eight ionization energies for a
particular neutral atom. All values are expressed in MJ
mol¯1. How many valence electrons does this atom
(A) 0
41. When the elements C, N and Si are arranged in order
of increasing first ionization energy, which is the correct
A. C < N < Si
C. Si < C < N
sigma bonds pi bonds lone pairs of electrons
10.99 13.33 71.33 84.01
(A) ionization energy
(C) electron affinity
(B) bond dissociation energy
(D) electronegativity
48. One way of writing the Lewis structure of the
cyanate ion, OCN¯, places one double bond between the
carbon atom and the oxygen atom and another double
bond between the carbon atom and the nitrogen atom.
What are the formal charges on the oxygen, carbon, and
nitrogen atoms, respectively for this structure?
(A) 0, 0, -1
(C) -1, +1, -1
(B) -1, 0, 0
(D) -2, 1, 0
49. Which pair are two different names for the same
43. Which gaseous ion in its ground state has the
greatest number of unpaired electrons?
(A) acetic acid and ethanoic acid
(B) formaldehyde and methanol
(C) isopropyl alcohol and 1-propanol
(D) ethene and ethyne
A. Mn3+
50. High solubility of an ionic solid in water is
A. 1
B. 2
C. 4
B. Fe3+
D. 6
C. Co3+
D. Ni3+
44. Which of these characteristics describe the
PCl3 molecule?
I trigonal planar shape
II sp3 hybridized phosphorus atom
III polar bonds
IV nonpolar molecule
A. I and II only
C. I and IV only
B. II and III only
D. I, III, and IV only
45. According to the Lewis structure for the HNNH,
how many sigma bonds, pi bonds, and lone pairs of
electrons are present?
favored by which of the following conditions?
I. The existence of strong ionic attractions in the
crystal lattice
II. The formation of strong ion-dipole attractions
III. An increase in entropy upon dissolving
(A) I only
(C) II only
(B) I and II only
(D) II and III only