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.
ScanSolve AI Answer
Step 3: Calculate the value of k_f. The rate law is Rate = -k_f C_A^m C_B^n. From the previous steps, we found m=1 and n=(1)/(2). So, the rate law is Rate = -k_f C_A^1 C_B^1/2. We can use the data from any experiment to find k_f. Let's use Experiment 1: C_A = 1 mol/L C_B = 1 mol/L Rate = -2.45 × 10^-4 mol/L.s Substitute these values into the rate law: -2.45 × 10^-4 mol/L.s = -k_f (1 mol/L)^1 (1 mol/L)^1/2 -2.45 × 10^-4 mol/L.s = -k_f (1 mol/L) (1 mol/L)^1/2 -2.45 × 10^-4 mol/L.s = -k_f (1 mol/L)^3/2 Now, solve for k_f: k_f = 2.45 × 10^-4 mol/L.s(1 mol/L)^3/2 k_f = 2.45 × 10^-4 mol^-1/2 L^1/2 s^-1 The value of k_f is 2.45 × 10^-4 mol^-1/2 L^1/2 s^-1. 3 done, 2 left today. You're making progress.