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 1: Find m using experiments 1 and 2. The rate law is rate = -k_f C_A^m C_B^n. Using the data from Experiment 1 and Experiment 2: (Rate_2)/(Rate_1) = -k_f C_A,2^m C_B,2^n-k_f C_A,1^m C_B,1^n Substitute the values: -4.90 × 10^-4 mol/L.s-2.45 × 10^-4 mol/L.s = (2 mol/L)^m (1 mol/L)^n(1 mol/L)^m (1 mol/L)^n 2 = ((2)/(1))^m ((1)/(1))^n 2 = 2^m · 1^n 2 = 2^m Therefore, m = 1. The order of reaction with respect to A is 1. Step 2: Find n using experiments 2 and 3. Using the data from Experiment 2 and Experiment 3: (Rate_3)/(Rate_2) = -k_f C_A,3^m C_B,3^n-k_f C_A,2^m C_B,2^n Substitute the values and the value of m=1: -4.90 × 10^-4 mol/L.s-4.90 × 10^-4 mol/L.s = (1 mol/L)^1 (4 mol/L)^n(2 mol/L)^1 (1 mol/L)^n 1 = (1 · 4^n)/(2 · 1) 1 = (4^n)/(2) 2 = 4^n Since 4 = 2^2, we can write: 2^1 = (2^2)^n 2^1 = 2^2n Equating the exponents: 1 = 2n n = (1)/(2) The order of reaction with respect to B is (1)/(2) . That's 2 down. 3 left today — send the next one.