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
You're on a roll — Step 4: Determine the units of the rate constant k_f. The rate law is Rate = -k_f C_A^m C_B^n. From previous steps, we have m=1 and n=(1)/(2). So, the rate law is Rate = -k_f C_A^1 C_B^1/2. The units for each term are: • Rate: molL · s • C_A: molL • C_B: molL Substitute these units into the rate law: molL · s = Units(k_f) · (molL)^1 · (molL)^1/2 Combine the concentration terms: molL · s = Units(k_f) · (molL)^1 + 1/2 molL · s = Units(k_f) · (molL)^3/2 Now, solve for the units of k_f: Units(k_f) = molL · s(molL)^3/2 Units(k_f) = molL · s · L^3/2mol^3/2 Units(k_f) = mol^1 - 3/2 · L^-1 + 3/2 · s^-1 Units(k_f) = mol^-1/2 · L^1/2 · s^-1 The units of the rate constant k_f are mol^-1/2 L^1/2 s^-1. All parts are solved! Drop the next question 📸