Question

C= C HC c= нен н сн, cis-2-butene irans-2-butene 3. The half-life (t1) of the catalyzed isomerization of cis-2-butene gas to produce trans-2-butene gas, represented above, was measured under various conditions, as shown in the table below. Trial Number Initial Peis-2-bultene (torr) VL T (K) 112 (5) 300. 2.00 350. 100. 2 600 2.00 350. 100. 4.00 350. 100. 300. 2.00 365 50. 300. a. The reaction is first order. Explain how the data in the table are consistent with a first-order reaction. b. Calculate the rate constant, k, for the reaction at 350. K. Include appropriate units with your answer. c. Is the initial rate of the reaction in trial 1 greater than, less than, or equal to the initial rate in trial 2? Justify your answer. d. The half-life of the reaction in trial 4 is less than the half-life in trial 1. Explain why, in terms of activation energy.

Answer 1

{ wiele like metode to predict outil @ca) (4.) - 90 m order Half life method to predict of the reaction 2 Yty)) - sa at ta' Stral-t, th, 510 trial - 2 the 100 n = It m(ho In (6) Forder n = 1t - 1 (feast order) Again Az = 0.693 (first order) & kr 0.693 is for Trial 1 k - 0.693 = 6.93 x1037 For Trial 2 lo For & 0.693 - 6.930103 gt Trial 3 k=0.693 – 6.934103 gt 100

6 Rate constant k. when T= 350k At = 350k on Trial 1, 2,3} ty=1005 2 ist order So, ta 0.693 ork-0.693 -0.693 -6.93x10 - 100$ Initial rate for trial-1 Sok, Po, = 6.93x108 [300 tors - 20079 toros Initial rate for trial-2 8 = K, Poz = 6.93 x1035 x (600) toor - 4.158 tools So intial rate of trial-1 is less than initial rate of trial-2. as pressure of initial rate trial I is les than trial 2.

As Temperature increases, the rate of reaction increases, due to increase in sate constant. Rate constant always dependent upon the temperature. Accordings to collision theory, Encrease in small in temperature rise to large increase in rate constant (increase in kinetic energy. If half life is lees then rate constant will be more. So trial-u has lees half life than trial-l. Energy Barrier -Activation energy Reactant Product 7 Reaction to-oodinate The temperature increases the kinetic energy or energy of system that can easily reach the energy barrier and reactant can converted in to product.