1002_1st Exam_1010321
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Consider the following reaction:
POCl3(g) POCl(g) + Cl2(g) Kc = 0.450
A sample of pure POCl3(g) was placed in a reaction vessel and allowed to decompose according to the above reaction. At equilibrium, the concentrations of POCl(g) and Cl2(g) were each 0.150 M. What was the initial concentration of POCl3(g)?
A) 0.633 M B) 0.225 M C) 0.350 M D) 0.200 M E) 0.483 M
Answer: D
2) Which statement is INCORRECT
A) The activated complex will be the highest on the energy profile.
B) In an endothermic reaction, activation energy is usually greater than the enthalpy.
C) If the forward reaction is exothermic, the reverse will be endothermic.
D) Activation energy is the same for forward and reverse reaction.
E) An activated complex has higher energy than any molecule contributing to it.
Answer: D
3) Which indication of relative acid strengths is INCORRECT?
A) HCl > HF B) HClO2 > HClO
C) CH3CO2H > CH3CH2OH D) H2SO3 > HNO3
E) H2SO4 > H2SO3 Answer: D
4) Consider the equilibrium system: N2O4(g) 2NO2(g) for which Kp = 0.1134 at 25°C and H°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container, compute PN2O at equilibrium.
A) 7.98 atm B) 1.01 atm C) 1.12 atm D) 8.88 atm E) 8.99 atm
Answer: B
5) What is the pH of a 0.563 M solution of ethylammonium bromide? Kb (ethylammonia) = 4.3 × 10-4
A) 5.32 B) 8.58 C) 5.44 D) 8.68 E) 1.79
Answer: C
6) What is the pH of a 0.253 M solution of ammonium chloride? Kb (NH3) = 1.2 × 10-5
A) 2.7 B) 11.3 C) 4.8 D) 9.9 E) 9.2
Answer: C
7) For a reaction Rate = k[A][B]2, what factor will keep k unchanged?
A) adding catalyst B) adding inhibitor
C) increasing [A] D) raising temperature
Answer: C
8) For 2 NO2(g) N2O4(g), Kc = [N2O4]/[NO2]2. At equilibrium there are 0.0270 mol N2O4 and 0.450 mol NO2 in a 50.0-L container. What is Kc?
A) 6.67 B) 0.133 C) 0.00267 D) 6.81 E) 2.45
Answer: A
9) For the reaction: C2H4Br2 + 3 KI C2H4 + 2 KBr + KI3, when the rate of reaction is 2.0 × 10-5, what is the rate of appearance of C2H4?
A) 0.67 × 10-5 B) 6.0 × 10-5 C) 2.0 × 10-5 D) 4.0 × 10-5 E) 1.0 × 10-5 Answer: C
10) 0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution with pH = 2.13. Determine the ionization constant of the acid.
A) 8.9 × 10-2 B) 3.6 × 10-6 C) 3.9 × 10-2 D) 6.6 × 10-4 E) 7.9 × 10-3 Answer: D
11) For the reaction 2 NO(g) N2O4(g) Kp equals ________.
A) Kc/RT B) Kc C) RT/Kc D) Kc(RT) E) Kc(RT)2
Answer: A
12) What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?
A) 10-4 M B) 10-8 M C) 10-12 M D) 10-2 M E) 10-5 M
Answer: D
13) Given the following initial rate data, calculate the specific rate constant.
Experiment [A]o, M [B]o, M Initial rate, M/s
1 5.1 × 10-4 0.35 × 10-4 3.4 × 10-8
2 5.1 × 10-4 0.70 × 10-4 6.8 × 10-8
3 5.1 × 10-4 0.18 × 10-4 1.7 × 10-8
4 1.0 × 10-3 0.35 × 10-4 6.8 × 10-8
5 1.5 × 10-3 0.35 × 10-4 10.2 × 10-8
A) 3.6 M2s-1 B) 3.6 M2s-1 C) 1.9 M2/s2 D) 1.1 × 108 M2/s2
E) 1.9 M-1· s-1 Answer: E
14) What is the indication of the relative base strengths of the following bases?
CH3NH2 CHBr2NH2 CH2BrNH2
A) CH2BrNH2 > CHBr2NH2 > CH3NH2 B) CHBr2NH2 > CH3NH2 > CH2BrNH2 C) CHBr2NH2 > CH2BrNH2 > CH3NH2 D) CH2BrNH2 > CH3NH2 > CHBr2NH2 E) CH3NH2 > CH2BrNH2 > CHBr2NH2 Answer: E
15) What is the order of reaction for the following reaction: Rate = k[A]-1/2 [B]1/2 ? A) 1/2 order
B) zero order C) -1/2 order D) second order
E) first order Answer: B
16) For which of the following reactions does Kp = Kc?
A) 2SO2(g) + O2(g) 2SO3(g) B) C(s) + H2O(g) CO(g) + H2(g) C) H2(g) + I2(s) 2HI(g) D) 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g) Answer: D
17) List the following acids in order of increasing strength:
HClO2 HClO3 HClO4
A) HClO3 < HClO2 < HClO4 B) HClO4 < HClO2 < HClO3 C) HClO4 < HClO3 < HClO2 D) HClO2 < HClO3 < HClO4 E) HClO2 < HClO4 < HClO3 Answer: D
18) What is the rate law for the following mechanism?
N2O + NO N2ONO (Slow) N2ONO N2 + NO2 (Fast) A) Rate = k[N2][NO2]
B) Rate = k[NO]
C) Rate = k[N2ONO]
D) Rate = k[N2O][NO]
E) Rate = k[N2O]
Answer: D
19) A factor that decreases the activation energy for a reaction:
I) decreases the rate constant II) increases the rate constant III) has no effect on the rate constant IV) makes the product yield increase V) might be a catalyst
A) IV and III B) II and V C) II and IV D) I, IV, and V E) I and IV Answer: B
20) For CO2(g) + H2(g) CO(g) + H2O(g), Kc = [CO][H2O]/[CO2][H2], if there are 1.43 mols each of CO and H2, 0.572 mol H2 and 4.572 mols CO2, in a 4.0 L container at equilibrium, what is Kc?
A) 0.782 B) 0.137 C) 1.28 D) 0.547 E) 2.34
Answer: A
21) Which of the following statements is INCORRECT?
A) In a zero order reaction the rate remains constant throughout the reaction.
B) For a first order reaction ln [A]t/[A]o = kt.
C) Half-life in a first order reaction is constant.
D) Radioactive decay is a first order reaction.
E) In gaseous reactions [A] can be expressed as concentration or as pressure.
Answer: B
22) For the second order reaction A products, the following data are obtained:
[A] = 1.512 M, t = 0 min [A] = 1.490 M, t = 1.0 min [A] = 1.469 M, t = 2.0 min
What is the rate constant, k, for the reaction?
A) 2.2 × 10-2 M-1 min-1 B) 1.0 × 10-2 M-1 min-1 C) 3.6 × 10-3 M-1 min-1 D) 9.7 × 10-3 M-1 min-1 E) 1.4 × 10-2 M-1 min-1 Answer: D
23) A mixture containing 0.392 M A(g) and 0.452 M B(g) is allowed to come to equilibrium at 300 K. The reaction 3 A(g) + 2 B(g) C(g) + D(g) occurs. At equilibrium, [C] = 0.00128 M. What is the value of Kc?
A) 7.19 × 106 B) 1.39 × 10-4 C) 9.24 × 10-6 D) 1.36 × 102 E) 7.35 × 10-3 Answer: B
24) Which of the following keep the equilibrium position unchanged?
A) pressure change B) temperature decrease
送分
25) Choose the Br nsted-Lowry acids and bases in the following equation:
HCO3- + OH- H2O + CO32-
A) acids HCO3-, H2O bases OH-, CO32- B) acids H2O, CO32- bases HCO3-, OH- C) acids H2O, OH- bases HCO3-, CO32- D) acids HCO3-, OH- bases CO32-, H2O
E) acids OH-, CO32- bases HCO3-, H2O Answer: A
26) 4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction:
Br2(l) + Cl2(g) 2BrCl(g)
At the point of equilibrium there were 82.63 g of Br2(l). Compute the value of Kc for this reaction.
A) 0.0699 B) 3.50 C) 0.699 D) 0.849 E) 0.0849
Answer: A
27) At 35°C, Kp = 0.315 for the reaction N2O4(g) 2 NO2(g), if the initial pressure of NO2(g) in a container is 3.00 atm, what is the equilibrium pressure of N2O4(g)?
A) 0.685 atm B) 0.471 atm C) 0.315 atm D) 1.19 atm E) 1.88 atm
Answer: D
28) Which species in the following reaction acts as a Lewis acid?
CuSO4(s) + 4NH3(aq) [Cu(NH3)4]2+(aq) + SO42-(aq) A) SO42-
B) NH3 C) Cu2+
D) [Cu(NH3)4]2+(aq)
E) [Cu(NH3)4]2+(aq) and SO42- Answer: C
29) Which of the following is FALSE for a second order reaction?
A) 1/[A]t - 1/[A]o = kt.
B) If 1/[A] versus time is a straight line, the reaction is second order.
C) Each successive half-life is 4 times as long as the previous.
D) The slope of 1/[A]t versus time is k.
E) t1/2 = 1/k[A]o.
Answer: C
30) Write the equilibrium expression Kc for the reaction:
sodium sulfite(aq) + chloric acid (aq) sodium chlorite(aq) + sulfur dioxide(g) + water(l).
A) [NaClO3]2 [Na2SO3][HClO3]2 B) [NaClO3][SO2][H2O]
[Na2SO3][HClO3]
C) [NaClO3][SO2]
[Na2SO3][HClO3]
D) [NaClO3]2[SO2]
[Na2SO3][HClO3]2 E) [NaClO3]2[SO2][H2O]
[Na2SO3][HClO3]2 Answer: D
31) What is the pH of a 0.250 M solution of formic acid? Ka = 1.8 × 10-4
A) 0.60 B) 5.4 C) 2.2 D) 11.8 E) 8.6
Answer: C
32) Substance A decomposes by a first-order reaction. Starting initially with [A] = 2.00 M, after 150 min [A] = 0.50 M. For this reaction what is t1/2?
A) 75.0 min B) 300 min C) 150 min D) 37.5 min E) 15.0 min
Answer: A
33) The concept of an acid not limited to H+ or species containing one or more protons is inherent in:
A) both the Arrhenius and the Br nsted-Lowry theories B) both the Br nsted-Lowry and the Lewis theories C) only the Br nsted-Lowry theory
D) only the Arrhenius theory E) only the Lewis theory Answer: E
34) Which of the following lowers the activation energy of a reaction?
A) adding reactants B) removing products C) adding a catalyst D) raising the temperature
E) lowering the temperature Answer: C
35) Which of the following is a logical inference from the fact that a 0.10 molar solution of potassium acetate,
36) A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca2+] of such a solution?
A) 8.9 × 10-3 B) 5.6 × 10-13 C) 0.018 D) 2.3 × 10-5 E) 0.035
Answer: A
37) For the reaction: 2N2O5(g) 4NO2(g) + O2(g) the rate law is:
[O2]
t =k[N2O5]
At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol. What is the rate constant at 310 K?
A) 1.05 × 10-4 s-1 B) 7.29 × 10-6 s-1 C) 3.70 × 10-5 s-1 D) 2.78 × 10-5 s-1 E) 7.29 × 10-8 s-1 Answer: B
38) Write the equilibrium constant expression for the reaction:
3 Sn(s) + 4 HNO3(aq) + H2O(l) 3 H2SnO3(s) + 4 NO(g) A) Kc = [NO]4
[HNO3]4
B) Kc = [H2SnO3]3[NO]4 [HNO3]4 C) Kc =[H2SnO3]3[NO]4
[Sn]3[HNO3]4 D) Kc = [H2SnO3]3[NO]4
[Sn]3[HNO3]4[H2O]
E) Kc = [H2SnO3][NO]- [Sn][H2O][HNO3]
Answer: A 39) Define rate law
A) A theoretical equation that describes how the rate of reaction depends on temperature, orientation and number of collisions.
B) A theoretical equation that describes how the rate of reaction depends on the concentration of reactants.
C) An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants.
D) An experimentally determined equation that describes how the rate of reaction depends on temperature, orientation and number of collisions.
Answer: C
1020318 更正答案為 A
40) Consider the reaction:
2SO2(g) + O2(g) 2SO3(g) H° = -196.6 kJ/mol The equilibrium is displaced to the left if:
A) the temperature is raised B) some sulfur trioxide is removed C) some sulfur dioxide is added D) the pressure is raised
E) the temperature is lowered Answer: A
