Question:
Which of the following statements is NOT true for a reaction having rate law $r = k [\text{H}_2][\text{I}_2]$?
Which of the following statements is NOT true for a reaction having rate law $r = k [\text{H}_2][\text{I}_2]$?
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When an exponent is omitted in a rate law equation, it is implicitly equal to 1. To find the overall order instantly, just sum up all the hidden ones: $1 + 1 = 2$.
Updated On: Jun 18, 2026
- The reaction is first order in $\text{H}_2$
- Overall order of reaction is 1
- The reaction is first order in $\text{I}_2$
- Overall order of reaction is 2
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Question:
The question asks us to identify the false statement regarding a chemical reaction that possesses the experimental rate law equation $r = k [\text{H}_2][\text{I}_2]$.
Step 2: Key Formula or Approach:
For a general rate law expression $r = k [A]^x [B]^y$, the exponent $x$ denotes the order with respect to reactant $A$, the exponent $y$ denotes the order with respect to reactant $B$, and the sum of the exponents ($x + y$) defines the overall reaction order.
Step 3: Detailed Explanation:
Given the rate law: $$r = k [\text{H}_2]^1 [\text{I}_2]^1$$ The exponent of $[\text{H}_2]$ is 1, which means the reaction is of the first order with respect to $\text{H}_2$ (Statement A is correct). The exponent of $[\text{I}_2]$ is 1, which means the reaction is of the first order with respect to $\text{I}_2$ (Statement C is correct). The overall order of the reaction is calculated by summing these individual exponents: $\text{Overall Order} = 1 + 1 = 2$ (Statement D is correct). Therefore, statement (B), which claims that the overall order of the reaction is 1, is completely false.
Step 4: Final Answer:
The statement that is NOT true is option (B).
The question asks us to identify the false statement regarding a chemical reaction that possesses the experimental rate law equation $r = k [\text{H}_2][\text{I}_2]$.
Step 2: Key Formula or Approach:
For a general rate law expression $r = k [A]^x [B]^y$, the exponent $x$ denotes the order with respect to reactant $A$, the exponent $y$ denotes the order with respect to reactant $B$, and the sum of the exponents ($x + y$) defines the overall reaction order.
Step 3: Detailed Explanation:
Given the rate law: $$r = k [\text{H}_2]^1 [\text{I}_2]^1$$ The exponent of $[\text{H}_2]$ is 1, which means the reaction is of the first order with respect to $\text{H}_2$ (Statement A is correct). The exponent of $[\text{I}_2]$ is 1, which means the reaction is of the first order with respect to $\text{I}_2$ (Statement C is correct). The overall order of the reaction is calculated by summing these individual exponents: $\text{Overall Order} = 1 + 1 = 2$ (Statement D is correct). Therefore, statement (B), which claims that the overall order of the reaction is 1, is completely false.
Step 4: Final Answer:
The statement that is NOT true is option (B).
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