122ch14f - 57 14.84) 58 14.84) a) (cont.) 59 14.84) a)...

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57 14.84)
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58 14.84) a) (cont.)
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59 14.84) a) (cont.) c) Use the rate law to find the rate [HgCl 2 ] = 0.050 M [C 2 O 4 2 & ] = 0.10 M r = k [HgCl 2 ] [C 2 O 4 2 & ] 2 r = (8. 6 72 x 10 & 3 M -2 s -1 ) [0.050 M] [0.10 M] 2 r = 4.336 x 10 & 6 M/s = 4.3 x 10 & 6 M/s
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60 14.90) Use the Arrhenius equation that relates k to E a and T. k = A e & Ea/RT where, A = frequency factor E a = activation energy T = temperature of Kelvin a) Even if Ea rx1 = Ea rx2 the k’s do NOT have to be equal. The rate constant, k, also depends on A, the frequency factor, which is related to the frequency of collisions and their effectiveness (proper orientation). So if A rx1 A rx2 then k rx1 k rx2 b) Two similar reactions have the same rate constant at 25°C, but at 35°C one of the reactions has a higher rate constant than the other. Why? From the two-point form of the Arrhenius equation one sees that the temperature dependance of the rate constant, k, depends on the activation energy, E a . Reactions with different behaviors for k with respect to temperature must have different activation energies, E a . The fact the two reactions have the same rate constant at 25°C is a coincidence.
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122ch14f - 57 14.84) 58 14.84) a) (cont.) 59 14.84) a)...

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