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
Here's how to solve this problem: Step 1: Identify the given information. The reaction is first order. The concentration of the reactant, [N_2O_5] = 0.01 mol/dm^3. The specific rate constant, k = 2.0 × 10^-3 s^-1. Step 2: Calculate the rate of reaction. For a first-order reaction, the rate law is: Rate = k[N_2O_5] Substitute the given values: Rate = (2.0 × 10^-3 s^-1) × (0.01 mol/dm^3) Rate = 2.0 × 10^-5 mol dm^-3 s^-1 The rate of reaction is 2.0 × 10^-5 mol dm^-3 s^-1. Step 3: Calculate the half-life. For a first-order reaction, the half-life (t_1/2) is given by the formula: t_1/2 = (0.693)/(k) Substitute the value of k: t_1/2 = (0.693)/(2.0 × 10^-3) s^-1 t_1/2 = 346.5 s The half-life is 346.5 s. Drop the next question 📸