Initial rate data is collected for the reaction . Exp 1: . Exp 2: . Exp 3: . Exp 4: . What is the ex — Chemical Kinetics Chemistry Question
Question
Initial rate data is collected for the reaction $A + B \rightarrow C$. Exp 1: $[A]=0.012\text{ M}, [B]=0.035\text{ M}, \text{Rate}=0.10 \text{ M s}^{-1}$. Exp 2: $[A]=0.024\text{ M}, [B]=0.070\text{ M}, \text{Rate}=1.6 \text{ M s}^{-1}$. Exp 3: $[A]=0.024\text{ M}, [B]=0.035\text{ M}, \text{Rate}=0.20 \text{ M s}^{-1}$. Exp 4: $[A]=0.012\text{ M}, [B]=0.070\text{ M}, \text{Rate}=0.80 \text{ M s}^{-1}$. What is the experimentally determined rate law?
💡 Solution & Explanation
Comparing Exp 1 and Exp 3: When $[A]$ is doubled and $[B]$ is kept constant, the rate doubles ($0.10 \rightarrow 0.20$). Thus, the order with respect to $A$ is $1$. Comparing Exp 1 and Exp 4: When $[B]$ is doubled and $[A]$ is kept constant, the rate becomes 8 times ($0.10 \rightarrow 0.80$). Thus, the order with respect to $B$ is $3$. The rate law is $\text{Rate} = k[A][B]^3$.