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Name: ________________________ Class: ___________________ Date: __________ Chapter 14 Practice test Multiple Choice Identify the choice that best completes the statement or answers the question. ____ 1) A burning splint will burn more vigorously in pure oxygen than in air because ________. A) oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than is in air B) oxygen is a catalyst for combustion C) oxygen is a product of combustion D) nitrogen is a product of combustion and the system reaches equilibrium at a lower temperature E) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the combustion The data in the table below were obtained for the reaction: A+BP Experiment Number 1 2 3 ____ [A](M) [B](M) 0.273 0.273 0.819 0.763 1.526 0.763 Initial Rate (M/s) 2.83 2.83 25.47 2) The rate law for this reaction is rate = ________. A) k[A][B] B) k[P] C) k[A]2[B] D) k[A]2[B]2 E) k[A]2 The data in the table below were obtained for the reaction: 2 ClO2 (aq) + 2 OH– (aq) ClO3– (aq) + ClO2– (aq) + H2O (1) ____ 3) What is the overall order of the reaction? A) 4 B) 0 C) 1 D) 2 E) 3 1 ID: A Name: ________________________ ____ ID: A 4) The reaction CH3–N=C CH3–C=N is a first-order reaction. At 230.3 °C, k = 6.29 10–4s–1. If is 1.00 10–3 initially, ________ after 1.000 103 s. A) 5.33 10–4 B) 2.34 10–4 C) 1.88 10–3 D) 4.27 10–3 E) 1.00 10–6 ____ 5) The following reaction is second order in [A] and the rate constant is 0.025 M –1s–1: A B The concentration of A was 0.65 M at 33 s. The initial concentration of A was ________ M. A) 2.4 B) 0.27 C) 0.24 D) 1.4 E) 1.2 10–2 ____ 6) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) CH3CN (g) The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C. The rate constant for the reaction is ________ s –1. A) –1.9 104 B) +1.9 104 C) –5.2 10–5 D) +5.2 10–5 E) +6.2 2 is Name: ________________________ ____ ID: A 7) Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction? A) B) C) D) E) x y x+y x–y y–x ____ 8) In general, as activation energy increases, reaction rate ________. A) goes down if the reaction is exothermic B) goes down if the reaction is endothermic C) stays the same regardless of whether the reaction is exothermic or endothermic D) goes down regardless of whether the reaction is exothermic or endothermic E) none of the above ____ 9) A possible mechanism for the overall reaction Br2 (g) + 2NO (g) 2NOBr (g) is NO (g) + Br2 (g) NOBr2 (g) + NO (g) NOBr2 (g) 2NOBr (fast) (slow) The rate law for formation of NOBr based on this mechanism is rate = ________. A) k1[NO]1/2 B) k1[Br2]1/2 C) (k2k1/k–1)[NO]2[Br2] D) (k1/k–1)2[NO]2 E) (k2k1/k–1)[NO][Br2]2 ____ 10) A catalyst can increase the rate of a reaction ________. A) by changing the value of the frequency factor (A) B) by increasing the overall activation energy (E a) of the reaction C) by lowering the activation energy of the reverse reaction D) by providing an alternative pathway with a lower activation energy E) All of these are ways that a catalyst might act to increase the rate of reaction. 3 Name: ________________________ ID: A ____ 11) The active site of nitrogenase is a cofactor that contains two transition metals. These transition metals are ________. A) Cr and Mg B) Mn and V C) Os and Ir D) Fe and Zn E) Fe and Mo ____ 12) Consider the following reaction: A 2C The average rate of appearance of C is given by [C]/t. Comparing the rate of appearance of C and the rate of disappearance of A, we get [C]/t = ________ (–[A]/t). A) +2 B) –1 C) +1 D) +1/2 E) –1/2 A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) B(g). The following data are obtained for [A] as the reaction proceeds: ____ 13) The average rate of disappearance of A between 20 s and 30 s is ________ mol/s. A) 5.0 10–4 B) 1.6 10–2 C) 1.5 10–3 D) 670 E) 0.15 4 Name: ________________________ ID: A The peroxydisulfate ion (S 2O82–) reacts with the iodide ion in aqueous solution via the reaction: S2O82– (aq) + 3I– 2SO4 (aq) + I3– (aq) An aqueous solution containing 0.050 M of S 2O82– ion and 0.072 M of I – is prepared, and the progress of the reaction followed by measuring [I–]. The data obtained is given in the table below. ____ 14) The average rate of disappearance of I– in the initial 400.0 s is ________ M/s. A) 6.00 B) 3.8 10–5 C) 1.4 10–4 D) 2.7 104 E) 3.2 10–4 ____ 15) The concentration of S2O82– remaining at 1600 s is ________ M. A) 0.036 B) 0.014 C) 0.043 D) 0.064 E) 0.029 ____ 16) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) CH3CN (g) At the start of the experiment, there are 0.200 mol of reactant (CH 3NC) and 0 mol of product (CH3CN) in the reaction vessel. After 25 min of reaction, 0.108 mol of reactant (CH 3NC) remain. The average rate of decomposition of methyl isonitrile, CH3NC, in this 25 min period is ________ mol/min. A) 3.7 10–3 B) 0.092 C) 2.3 D) 4.3 10–3 E) 0.54 ____ 17) The overall order of a reaction is 1. The units of the rate constant for the reaction are ________. A) M/s B) M–1s–1 C) 1/s D) 1/M E) s/M2 5 Name: ________________________ ID: A ____ 18) A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to ________. A) remain constant B) increase by a factor of 27 C) increase by a factor of 9 D) triple E) decrease by a factor of the cube root of 3 The data in the table below were obtained for the reaction: A + B P ____ 19) The overall order of the reaction is ________. A) 1 B) 2 C) 3 D) 4 E) 0 ____ 20) The half-life of a first-order reaction is 13 min. If the initial concentration of reactant is 0.13 M, it takes ________ min for it to decrease to 0.085 M. A) 12 B) 10. C) 8.0 D) 11 E) 7.0 ____ 21) The reaction below is first order in [H2O2]: 2H2O2 (l) 2H2O (l) + O2 (g) A solution originally at 0.600 M H 2O2 is found to be 0.075 M after 54 min. The half-life for this reaction is ________ min. A) 6.8 B) 18 C) 14 D) 28 E) 54 6 Name: ________________________ ID: A ____ 22) A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M. The rate constant for this reaction is ________ M –1s–1. A) 12 B) 2.0 10–2 C) 8.5 10–2 D) 4.3 10–2 E) 4.3 ____ 23) The reaction shown below is ________, and it is a ________ elementary reaction. A + B + C ABC A) termolecular, rare B) termolecular, common C) unimolecular, common D) bimolecular, rare E) unimolecular, rare ____ 24) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N2O5(g) 4NO2 (g) + O2 (g) When the rate of formation of O2 is 2.2 10–4 M/s, the rate of decomposition of N2O5 is ________ M/s. A) 7.2 10–3 B) 3.6 10–3 C) 1.8 10–3 D) 1.4 10–2 E) 0.00090 ____ 25) The combustion of ethylene proceeds by the reaction C2H4 (g) + 3O2 (g) 2CO2 (g) + 2H2O (g) When the rate of disappearance of O2 is 0.13 M s–1, the rate of disappearance of C2H4 is ________ M s–1. A) 0.087 B) 0.043 C) 0.39 D) 0.20 E) 0.26 ____ 26) In a linear graphical representation of a zero-order reaction, what value is represented by the y-intercept of the line drawn from plotting [A] vs. time? A) [A]0 B) ln[A]0 C) 1/[A]0 D) [A]02 E) [A]/k 7 Name: ________________________ ID: A ____ 27) The rate constant of a first-order process that has a half-life of 462 s is ________ s –1. A) 1.50 10–3 B) 3.20 102 C) 6.67 102 D) –1.08 10–3 E) 2.16 10–3 ____ 28) The elementary reaction 2NO2 (g) 2NO (g) + O2 (g) is second order in NO2 and the rate constant at 660 K is 5.23 M –1s–1. The reaction half-life at this temperature when [NO2]0 = 0.45 M is ________ s. A) 2.4 B) 7.6 C) 0.19 D) 0.13 E) 0.42 ____ 29) The rate constant for a particular second-order reaction is 0.47 M –1s–1. If the initial concentration of reactant is 0.25 mol/L, it takes ________ s for the concentration to decrease to 0.20 mol/L. A) 2.1 B) 1.4 C) 1.0 D) 0.47 E) 0.20 ____ 30) The rate constant for a second-order reaction is 0.13 M –1s–1. If the initial concentration of reactant is 0.26 mol/L, it takes ________ s for the concentration to decrease to 0.07 mol/L. A) 0.017 B) 1.4 C) 14 D) 80. E) 10. ____ 31) A particular first-order reaction has a rate constant of 1.35 102 s–1 at 25.0 °C. What is the magnitude of k at 65.0 °C if Ea = 55.5 kJ/mol? A) 1.92 103 B) 1.95 104 C) 358 D) 3.48 1073 E) 1.35 102 Short Answer 1) The relationship of absorbed light to the concentration of the substance absorbing the light is governed by ________. 8 Name: ________________________ ID: A 2) For the reaction aA + Bb cC + dD, the rate law is ________. 3) If a rate law is second order (reactant), doubling the reactant ________ the reaction rate. 4) The Earth's ozone layer is located in the ________. 5) Reaction rates are affected by reactant concentrations and temperature. This is accounted for by the ________. 6) The minimum energy to initiate a chemical reaction is the ________. 7) Reaction rate data showing temperature dependence obey an equation devised by ________. 8) The number of molecules that participate as reactants defines the ________ of the reaction. 9) Elementary reactions involving the simultaneous collision of three molecules are ________. 10) A catalyst that is present in the same phase as the reacting molecules is called a(n) ________ catalyst. 11) A catalyst that is present in a different phase from the reacting molecules is called a(n) ________ catalyst. 12) The binding of molecules to the surface of a catalyst is referred to as ________. 13) The uptake of molecules into the interior of another substance is referred to as ________. True/False Indicate whether the statement is true or false. ____ 1) Rates of reaction can be positive or negative. ____ 2) The instantaneous rate of a reaction can be read directly from the graph of molarity versus time at any point on the graph. ____ 3) The overall reaction order is the sum of the orders of each reactant in the rate law. ____ 4) Units of the rate constant of a reaction are independent of the overall reaction order. ____ 5) The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law. ____ 6) The rate of a second order reaction can depend on the concentrations of more than one reactant. ____ 7) The half-life for a first order rate law depends on the starting concentration. ____ 8) The rate limiting step in a reaction is the slowest step in the reaction sequence. ____ 9) Heterogeneous catalysts have different phases from reactants. 9 ID: A Chapter 14 Practice test Answer Section MULTIPLE CHOICE 1) ANS: OBJ: 2) ANS: OBJ: 3) ANS: OBJ: 4) ANS: OBJ: 5) ANS: OBJ: 6) ANS: OBJ: 7) ANS: OBJ: 8) ANS: OBJ: 9) ANS: OBJ: 10) ANS: OBJ: 11) ANS: OBJ: 12) ANS: OBJ: 13) ANS: OBJ: 14) ANS: OBJ: 15) ANS: OBJ: 16) ANS: OBJ: 17) ANS: OBJ: 18) ANS: OBJ: 19) ANS: OBJ: 20) ANS: OBJ: 21) ANS: OBJ: A 14.1; G2 E 14.3; G4 E 14.3; G4 A 14.4; G4 D 14.4; G3 D 14.4; G3 A 14.5; G3 D 14.5; G2 C 14.6; G2 D 14.7; G2 E 14.7; G2 A 14.2; G2 C 14.2; G4 B 14.2; G3 A 14.2; G3 A 14.2; G4 C 14.3; G2 B 14.3; G4 B 14.3; G3 C 14.4; G4 B 14.4; G4 PTS: 1 DIF: 1 REF: Page Ref: 14.1 PTS: 1 DIF: 3 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 1 REF: Page Ref: 14.5 PTS: 1 DIF: 1 REF: Page Ref: 14.5 PTS: 1 DIF: 3 REF: Page Ref: 14.6 PTS: 1 DIF: 1 REF: Page Ref: 14.7 PTS: 1 DIF: 1 REF: Page Ref: 14.7 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.4 PTS: 1 DIF: 4 REF: Page Ref: 14.4 1 ID: A 22) ANS: OBJ: 23) ANS: OBJ: 24) ANS: OBJ: 25) ANS: OBJ: 26) ANS: OBJ: 27) ANS: OBJ: 28) ANS: OBJ: 29) ANS: OBJ: 30) ANS: OBJ: 31) ANS: OBJ: C 14.4; G4 A 14.1; G4 A 14.2; G4 B 14.2; G4 A 14.4; G2 A 14.4; G4 E 14.4; G4 A 14.4; G4 D 14.4; G4 A 14.5; G4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 4 REF: Page Ref: 14.1 PTS: 1 DIF: 1 REF: Page Ref: 14.2 PTS: 1 DIF: 2 REF: Page Ref: 14.2 PTS: 1 DIF: 4 REF: Page Ref: 14.4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 2 REF: Page Ref: 14.4 PTS: 1 DIF: 1 REF: Page Ref: 14.4 PTS: 1 DIF: 4 REF: Page Ref: 14.5 PTS: 1 OBJ: 14.2; G2 2) ANS: k[A]m[B]n DIF: 1 REF: Page Ref: 14.2 PTS: 1 OBJ: 14.3; G2 3) ANS: quadruples DIF: 1 REF: Page Ref: 14.3 PTS: 1 OBJ: 14.3; G2 4) ANS: stratosphere DIF: 1 REF: Page Ref: 14.3 PTS: 1 OBJ: 14.4; G2 5) ANS: collision model DIF: 1 REF: Page Ref: 14.4 PTS: 1 OBJ: 14.5; G2 DIF: 1 REF: Page Ref: 14.5 SHORT ANSWER 1) ANS: Beer's Law 2 ID: A 6) ANS: activation energy PTS: 1 OBJ: 14.5; G2 7) ANS: Arrhenius DIF: 1 REF: Page Ref: 14.5 PTS: 1 OBJ: 14.5; G2 8) ANS: molecularity DIF: 1 REF: Page Ref: 14.5 PTS: 1 OBJ: 14.6; G2 9) ANS: termolecular DIF: 1 REF: Page Ref: 14.6 PTS: 1 OBJ: 14.6; G2 10) ANS: homogeneous DIF: 1 REF: Page Ref: 14.6 PTS: 1 OBJ: 14.7; G2 11) ANS: heterogeneous DIF: 2 REF: Page Ref: 14.7 PTS: 1 OBJ: 14.7; G2 12) ANS: adsorption DIF: 2 REF: Page Ref: 14.7 PTS: 1 OBJ: 14.7; G2 13) ANS: absorption DIF: 1 REF: Page Ref: 14.7 PTS: 1 OBJ: 14.7; G2 DIF: 3 REF: Page Ref: 14.7 PTS: 1 DIF: 1 REF: Page Ref: 14.2 PTS: 1 DIF: 1 REF: Page Ref: 14.2 PTS: 1 DIF: 1 REF: Page Ref: 14.3 TRUE/FALSE 1) ANS: OBJ: 2) ANS: OBJ: 3) ANS: OBJ: F 14.2; G2 F 14.2; G2 T 14.3; G2 3 ID: A 4) ANS: OBJ: 5) ANS: OBJ: 6) ANS: OBJ: 7) ANS: OBJ: 8) ANS: OBJ: 9) ANS: OBJ: F 14.3; G2 T 14.3; G2 T 14.4; G2 F 14.4; G2 T 14.6; G2 T 14.7; G2 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.3 PTS: 1 DIF: 1 REF: Page Ref: 14.4 PTS: 1 DIF: 1 REF: Page Ref: 14.4 PTS: 1 DIF: 1 REF: Page Ref: 14.6 PTS: 1 DIF: 1 REF: Page Ref: 14.7 4 Chapter 14 Practice test [Answer Strip] A _____ 4) A _____ 7) ID: A E 11) _____ A _____ 1) A 12) _____ B 14) _____ D _____ 5) D _____ 8) A 15) _____ C _____ 9) A 16) _____ D _____ 6) C 13) _____ E _____ 2) C 17) _____ D 10) _____ E _____ 3) Chapter 14 Practice test [Answer Strip] B 18) _____ C 22) _____ A 23) _____ ID: A A 27) _____ E 28) _____ A 24) _____ B 19) _____ A 29) _____ C 20) _____ B 25) _____ D 30) _____ F _____ 1) F _____ 2) B 21) _____ A 31) _____ T _____ 3) F _____ 4) A 26) _____ T _____ 5) T _____ 6) F _____ 7) T _____ 8) T _____ 9)
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