Read the statement and choose the option correctly.

Explanation

The general form of a rate law is: Rate =k[A]x[B]y1. Find the effect of changing [A] (Order with respect to A):Compare Experiment 1 and Experiment 2.In Experiment 1: [A]=0.1, [B]=0.1, Rate =2×10−5In Experiment 2: [A]=0.2, [B]=0.1, Rate =4×10−5Notice that [B] stays the same (0.1).When [A] doubles (from 0.1 to 0.2), the Rate also doubles (from 2×10−5 to 4×10−5).If doubling the concentration doubles the rate, the reaction is first order with respect to A. So, x=1.2. Find the effect of changing [B] (Order with respect to B):Compare Experiment 1 and Experiment 3.In Experiment 1: [A]=0.1, [B]=0.1, Rate =2×10−5In Experiment 3: [A]=0.1, [B]=0.2, Rate =4×10−5Notice that [A] stays the same (0.1).When [B] doubles (from 0.1 to 0.2), the Rate also doubles (from 2×10−5 to 4×10−5).If doubling the concentration doubles the rate, the reaction is first order with respect to B. So, y=1.3. Combine to find the Rate Law: Since x=1 and y=1, the rate law is: Rate =k[A]1[B]1 Which simplifies to: Rate =k[A][B]