(一) Multiple Choice(80﹪)
(1) Which of the following is an assumption of the kinetic molecular theory applied to gases?
(a) Molecules have definite volume. (b) Molecules of all gases have the same average velocity
at different temperature (c) Gas molecules have negligible repulsive forces (d) Different gases
have the different kinetic energy (e)All collisions involving gas molecules are not elastic …□
(2) Which of the following is a representation of Charles's law?
(a) P  1/V (b) V  P (c) V  T (d) P  1/T (e) V  1/T ………□
(3) Which of the following is a representation of Avogdro's law?
(a) P  1/V (b) V  n (c) V  T (d) V  1/n (e) P  T ………□
(4) The temperature of a volume of gas is decreased from 60℃ to 30℃ at constant pressure.
Its volume (a) doubles (b) increase by half (c) increase by a factor of 303/333 (d) decrease
by a factor of 30/333 (e) increase by a factor of 333/303 ……….□
(5) In which of the following is a representation of combined gas law? (a) P1T1/V1＝P2T2/V2
(b) P1V1/T1＝P2V2/T2(c)V1T1/P1＝V2T2/P2 (d) P1V2 /T1＝P2V1/T2(e) P1T2 /V1＝P2T1 /V2 .□
(6) Which of the following is the set of condition known as standard temperature and pressure
(STP)? (a) 0K and 1atm (b) 0℃ and 760torr (c) 273K and 760atm (d) 273℃ and 1atm
(e) 273K and 760torr …..□
(7) Which of the following gases has the lowest average velocity at a given temperature?
(a) Oxygen (b) Carbon monoxide (c) Helium (d) Sulfur dioxide (e) Hydrogen chloride ..□
(8) A mixture of gases has a total pressure of 4 atm. If one gas has a partial pressure of 1 atm,
what part of the mixture is this gas? (a) 50% (b) 75% (c) 25% (d) 100% (e) 20% ……□
(9) A 11.2 L quantity of He at STP (a) contains 0.5 mol of He atoms. (b) has the mass of 4 g.
(c) contains 6×1023 He atoms (d) contains 1 mol of He molecules (e) has a mass of 8 g ..□
(10) A gas has a density of 2.05g/L (STP). What is the gas?
(a) CO2 (b) SO2 (c) NO2 (d) COS (e) CO …….□
(11) Given the equation C(s) + H2O(l)  CO(g) + H2(g) What volume of gas measured at STP
would be produced from 6 g of carbon (a) 22.4L (b) 11.2L (c) 44.8L (d) 33.6L (e) 5.6L ..□
(12) Given the equation 2KClO3(s)  2KCl (s)+ 3O2 (g) What volume of gas measured at STP
would be produced from 122.5g of KClO3 (a) 22.4L (b) 11.2L (c) 44.8L (d) 33.6L (e) 5.6L□
(13) When the temperature decrease, solids generally become ____ soluble and gases become
____ soluble.(a) more, more (b) less, more (c) less, less (d) more, less (e) none …....□
(14) A 4 L quantity of 0.5 M HCl contains (a) 1.0 mol of HCl (b) 2.0 mol of H2O (c) 2.0 mol
of HCl (d) 1.0 mol of H2O (e) 0.5 mol of HCl ………□
(15) An experiment calls for 2.0 L of 0.1 M HCl, which must be prepared from 4.0 M HCl.
What volume in milliliters of the concentrated acid is needed to be diluted to form the
0.1 M solution (a) 400 mL (b) 200 mL (c) 100 mL (d) 250 mL (e) 50 mL ……….□
(16) Which of the following is not a colligative property (a) boiling point elevation (b) vapor
pressure lowering (c) freezing point depression (d) osmotic pressure elevation (e) none □
(17) What is the freezing point of a 1 m aqueous solution of a nonelectrolyte (H2O Kf = 1.86)
(a)－1.86℃ (b) 0.186℃ (c) －0.186℃ (d) 1.86℃ (e) －18.6℃ ……….□
(18) Compare to pure water, a 0.5 m aqueous sugar solution will have a ____ boiling point
a ____ vapor pressure, and a ____ freezing point, (a) higher, lower, lower (b) lower, higher,
higher (c) lower, lower, higher (d) lower, higher, lower (e) higher, lower, higher ……□
(19) If solutions of each of the following have the same concentration, which has the highest
boiling point (a) CH3OH(nonelectrolyte)(b) NaCl (c) Na2SO4 (d) CaS (e) all are the same□
(20) If solutions of each of the following have the same concentration, which has the lowest
freezing point (a) C6 H12 O6(nonelectrolyte)(b) CaSO4 (c) KNO3 (d) MgCl2 (e) CuS …..□
(21) What is the boiling point of a 0.5 m aqueous solution of NaCl (H2O Kb=0.52)
(a)100.26℃ (b)100.52℃ (c)101.04℃ (d)99.84℃ (e) 99.48℃ …….□
(22) A 2 L quantity of 0.1 M H2SO4 contains (a) 4.9 g of H2SO4 (b) 0.1mol of H2SO4 (c) 9.8 g
of H2SO4 (d) 0.5mol of H2SO4 (e) 19.6 g H2SO4 ………□
(23) What volume of 4.5 M NaOH should be diluted with water to from 3 L of 1.5 M base
(a) 250mL (b) 500 mL (c) 750 mL (d) 1000 mL (e) 1500 mL ………□
(24) If the water remains a nonconductor, the solute is a (a) nonelectrolyte (b) weak electrolyte
(c) electrolyte (d) strong electrolyte (e) none …………□
(25) Which of the following is an oxidation-reduction reaction? (a) Mg2＋＋CO32－  MgCO3
(b) HCl  H＋＋Cl－(c) H＋＋O H－  H2O (d) KOH  K＋＋O H－(e)Zn＋Cl 2  ZnCl2 ..□
(26) Which of the following is an reduction process? (a) 2Br－  Br2 (b) Fe2＋  Fe2O3
(c) S2－  SO42－(d)H2CO3  H2O＋CO2(e) P4  H3PO4 ………..□
(27) Which of the following is an oxidation process? (a) S2O82－  SO42－ (b) I2  2I－
(c)Zn 2＋  Zn (d)Al  Al(OH)4－ (e) NO3－  NH4＋ ………..□
(28) What is the oxidation state of the S in Al2(SO3)3 (a)+6 (b)+4 (c)+2 (d)－2 (e)－4 ……..□
(29) What is the oxidation state of the I in H5IO6 (a)+7 (b)+6 (c)+5 (d)－1 (e)+1……..□
(30) In the following electrolytic cell,___ is___ at the anode.2Br－(aq)+Ni 2＋(aq)  Br2(g)+Ni(s)
(a) Br－,oxidized (b) Br2 ,oxidized(c) Ni 2＋, reduced (d) Ni , oxidized(e) Br－,reduced ….□
(31) In the following electrolytic cell,__ is__ at the cathode.2Cl－(aq)+Fe 2＋(aq)  Cl2(g)+Fe(s)
(a) Cl－,oxidized (b) Cl2,oxidized(c) Fe 2＋, reduced (d) Fe, oxidized (e) Cl－,reduced …...□
(32) In the following equation , how many electrons have been gained(＋e－) or lost(－e－) by
one molecule of I2？ I2  IO3－(a)＋6(b)＋5 (c)＋2(d)－5 (e)－6 ………□
(二)Problem(40﹪)
(1) Given the following unbalanced equation. What volume of NO gas measured at STP is
produced by the complete of 14.3 g of Cu2O NO3－(aq)+H＋(aq)＋Cu2O (s)  Cu 2＋(aq)＋
NO (g)+ H2O(l)
(2) Given the following unbalanced equation. What mass of Zn is required to produce 2.8 g of
N2？ NO3－(aq)+H＋(aq)＋Zn (s)  Zn2＋(aq)＋N2 (g)+ H2O(l)
(3) Sketch a galvanic cell in which the following overall reaction occurs Cu(s)＋2Ag＋(aq) 
Cu2＋(aq)＋2Ag(s) What reaction take place at the anode and the cathode. In what direction
do the electrons flow in the wire. In what direction do the anions flow in the salt bridge.
(4) Describe how a voltaic cell could be constructed from a stripe of zinc, a stripe of nicle,a
Zn(NO3)2 solution, and a Ni(NO3)2 solution. Write the anode reaction and the cathode
reaction, and the total reaction.
Atomic mass
C:12, O:16, N:14, H:1, Zn:65, Cu:63.5, Cl:35.5, K:39, He:4, S:32