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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Here's a detailed breakdown of the solution based on your questions: The general rate law for the reaction A + B + C D is: 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. Step 1: Determine the order with respect to [B] (y) To find y, we compare experiments where [A] and [C] are constant, but [B] changes. Comparing Experiment 1 and Experiment 2: 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 = (0.01 M)^x(0.2 M)^y(0.02 M)^z(0.01 M)^x(0.01 M)^y(0.02 M)^z 1 = ((0.2)/(0.01))^y 1 = (20)^y This means y = 0. The reaction is zero order with respect to B. Step 2: Determine the order with respect to [C] (z) To find z, we compare experiments where [A] and [B] are constant, but [C] changes. Comparing Experiment 1 and Experiment 4: 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 = (0.01 M)^x(0.01 M)^y(0.02 M)^z(0.01 M)^x(0.01 M)^y(0.01 M)^z 2 = ((0.02)/(0.01))^z 2 = (2)^z This means z = 1. The reaction is first order with respect to C. Step 3: Determine the order with respect to [A] (x) To find x, we compare experiments where [B] and [C] are constant (or where changes in [B] don't affect the rate since y=0), but [A] changes. Comparing Experiment 1 and Experiment 3, using y=0 and z=1: Rate_3Rate_1 = (k[A]_3^x[B]_3^0[C]_3^1)/(k[A]_1^x[B]_1^0[C]_1^1) 0.018 M s^-10.006 M s^-1 = (0.03 M)^x(0.02 M)^0(0.02 M)^1(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 means x = 1. The reaction is first order with respect to A. --- 1. Write the rate law of the reaction Based on the orders determined (x=1, y=0, z=1): Rate = k[A]^1[B]^0[C]^1 Rate = k[A][C] 2. Derived the rate law This involves finding the orders of reaction for each reactant (as shown in Steps 1-3) and then calculating the rate constant (k). Using the rate law Rate = k[A][C] and data from Experiment 1: 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 3. Derived the order of the reaction The overall order of the reaction is the sum of the individual orders (x+y+z): Overall order = 1 + 0 + 1 = 2 The overall order of the reaction is: 2nd order What's next?