Question

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: Experiment [A] (M) [B] (M) Rate (M/s) 0.6 0.4 (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. [A] = 0.6 and [B] = 0.8 [A] = 1.2 and [B] = 1.2 [A] = 2.4 and [B] = 0.4 [A] = 0.6 and [B] = 1.2 [A] = 3.0 and [B] = 0.4 [A] = 1.2 and [B] = 0.4 [A] = 1.8 and [B] = 0.4 [A] = 1.2 and [B] = 0.8 (b) For a reaction of the form, A+B+C --> Products, the following observations are made: doubling the concentration of A increases the rate by a factor of 8, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 3. Select the correct rate law for this reaction from the choices below. Rate = K[A][B][C] Rate = K[A][C] Rate = k[A]2[C] Rate = k[A][C] Rate = k[A]? [C]2 Rate = k[A] [C] Rate = k[A][C]

Answer 1

Answer! - @ (AJ= 0.6 and [B] = 1.2 is used because [A] needs to be cancelled in order to get order with respect to B, while taking ratio. when [A ] is doubled rate increases by factor of 8 means order with respect to a meest be 3 as (213=8 Now AS B heas no effect ; so order=0 where order with respect to c meest be 1 ag concentraton is tripled rate algo tripled (311-3 .. Rate = K[Ay CB7° [C]' ... Rate = k CA² (c] (answer' ② Rate = k CAJ? (B] CCJ Rate douated when Ratezak [2A/3 ( 2 B30 (₂) concentration is halved Rate 1 donaten orginal note Rate, A3 XIXC Rate 2 0.125 A3 X I XO 5 Rate 1 1 Rate 2 0.125 x 0.5 Rate q = 0.0625 Rate 1. rate willl be the ongenal rate multiplied by a facter of 10.0625 So the