For a chemical reaction A B, it was found that concentration of B is increased by 0.2 mol L in 30 mi — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

**Step 1: Identify the given information** - Change in concentration of B: Δ[B] = 0.2 mol/L - Time interval: Δt = 30 min - Need to find: average rate in mol L⁻¹ h⁻¹ **Step 2: Apply the average rate formula** Average rate = Δ[concentration] / Δ[time] Average rate = 0.2 mol/L ÷ 30 min **Step 3: Calculate rate in mol L⁻¹ min⁻¹** Average rate = 0.2/30 = 1/150 mol L⁻¹ min⁻¹ **Step 4: Convert time from minutes to hours** Since 1 hour = 60 minutes: Average rate = (1/150 mol L⁻¹ min⁻¹) × 60 min/h Average rate = 60/150 = 0.4 mol L⁻¹ h⁻¹ **Step 5: Express in the required format (× 10⁻¹)** 0.4 mol L⁻¹ h⁻¹ = 4.0 × 10⁻¹ mol L⁻¹ h⁻¹ The coefficient is 4.00. Therefore, the answer is 4.00.