This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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The general rate law for the reaction A + B + C D is given by: Rate = k[A]^x[B]^y[C]^z where x, y, z are the orders of reaction with respect to A, B, and C, respectively, and k is the rate constant. Step 1: Determine the order with respect to [B] (y) Compare Experiment 1 and Experiment 2, where [A] and [C] are constant. Rate_2Rate_1 = (k[A]_2^x[B]_2^y[C]_2^z)/(k[A]_1^x[B]_1^y[C]_1^z) 0.006 M s^-10.006 M s^-1 = k(0.01 M)^x(0.2 M)^y(0.02 M)^zk(0.01 M)^x(0.01 M)^y(0.02 M)^z 1 = ((0.2)/(0.01))^y 1 = (20)^y This implies y = 0. The reaction is zero order with respect to B. Step 2: Determine the order with respect to [C] (z) Compare Experiment 1 and Experiment 4, where [A] and [B] are constant. Rate_1Rate_4 = (k[A]_1^x[B]_1^y[C]_1^z)/(k[A]_4^x[B]_4^y[C]_4^z) 0.006 M s^-10.003 M s^-1 = k(0.01 M)^x(0.01 M)^y(0.02 M)^zk(0.01 M)^x(0.01 M)^y(0.01 M)^z 2 = ((0.02)/(0.01))^z 2 = (2)^z This implies z = 1. The reaction is first order with respect to C. Step 3: Determine the order with respect to [A] (x) Compare Experiment 1 and Experiment 3. We know y=0 and z=1. Rate_3Rate_1 = (k[A]_3^x[B]_3^y[C]_3^z)/(k[A]_1^x[B]_1^y[C]_1^z) 0.018 M s^-10.006 M s^-1 = k(0.03 M)^x(0.02 M)^0(0.02 M)^1k(0.01 M)^x(0.01 M)^0(0.02 M)^1 3 = ((0.03)/(0.01))^x ((0.02)/(0.02))^1 3 = (3)^x (1) This implies x = 1. The reaction is first order with respect to A. Step 4: Write the rate law (Question 1 and part of Question 2) Using the determined orders x=1, y=0, z=1: Rate = k[A]^1[B]^0[C]^1 Rate = k[A][C] The rate law is: Rate = k[A][C] Step 5: Calculate the rate constant (k) (Remaining part of Question 2) Using data from Experiment 1: Rate = 0.006 M s^-1 [A] = 0.01 M [C] = 0.02 M 0.006 M s^-1 = k(0.01 M)(0.02 M) 0.006 M s^-1 = k(0.0002 M^2) k = 0.006 M s^-10.0002 M^2 k = 30 M^-1s^-1 The rate constant is: k = 30 M^-1s^-1 Step 6: Derive the overall order of the reaction (Question 3) The overall order of the reaction is the sum of the individual orders: Overall order = x + y + z = 1 + 0 + 1 = 2. The overall order of the reaction is: 2nd order Send me the next one 📸