51) A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K, what is the rate constant at 366 K? A) 12 s-1 B) 1.7 s-1 C) 0.58 s-1 D) 5.4 × 10-5 s-1 E) 1.9 × 10-4 s-1 52) A reaction is found to have an activation energy of 38.0 kJ/mol. If the rate constant for this reaction is 1.60 × 102 M-1s-1 at 249 K, what is the rate constant at 436 K? A) 2.38 × 105 M-1s-1 B) 1.26 × 103 M-1s-1 C) 7.94 × 104 M-1s-1 D) 4.20 × 105 M-1s-1 E) 3.80 × 104 M-1s-1 53) If the activation energy for a given compound is found to be 42.0 kJ/mol, with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 K? A) 2.9 × 10-4 s-1 B) 7.4 × 10-4 s-1 C) 1.4 × 109 s-1 D) 4.6 × 10 5 s-1 E) 3.5 × 103 s-1 54) If the activation energy for a given compound is found to be 103 kJ/mol, with a frequency factor of 4.0 × 1013 s-1, what is the rate constant for this reaction at 398 K? A) 1.2 s-1 B) 8.2 s-1 C) 3.9 × 1010 s-1 D) 1.7 × 1010 s-1 E) 2.5 × 107 s-1 55) A reaction has a rate constant of 6.0 × 10-3 L2 mol-2 s-1 at 10°C. If its activation energy is 84 kJ/mol, what is the value of the rate constant at 50°C? A) 4.8 L2mol-2s-1 B) 0.50 L2mol-2s-1 C) 0.018 L2mol-2s-1 D) 8.2 × 103 L2mol-2s-1 E) 0.84 L2mol-2s-1 56) Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism A2 ? 2Afast A + B → ABslow A) Rate = k[A][B] B) Rate = k[A2][B] C) Rate = k[A2][B]1/2 D) Rate = k[A2] E) Rate = k [A2]1/2[B] 57) A reaction occurs via the following sequence of elementary steps. What is the reaction intermediate? 1st step: A + 2B → 2C 2nd step: 2C → D A) A B) B C) C D) D E) There is no intermediate 58) Which of the following is a rate law for a reaction that is first order with respect to oxygen? A) rate = k [NO2] B) rate = k [NO2]2 [O2}1/2 C) rate = k [NO2] [O2}1/2 D) rate = k [NO2] [O2}1/2 [N2]1/2 E) rate = k [NO2]2 [O2} 59) A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? 1st step: A + B → 2C + Dslow 2nd step: C → Efast 3rd step: D → 2Ffast A) rate = k [C]2 [D] B) rate = k [A] [B] C) rate = k [E] [F]2 D) rate = k [E] E) rate = k [C] 60) Which of the following statements is true? A) The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. B) A catalyst raises the activation energy of a reaction. C) Rate constants are temperature dependent. D) The addition of a homogeneous catalyst does not change the activation energy of a given reaction. E) None of the above are true.