Q26 / 150 · MHT CET 2026 (11 April Shift 2) · Chemistry
What is the order of the following reaction ?
$2\text{H}_2\text{O}_2 (l) \rightarrow 2\text{H}_2\text{O} (l) + \text{O}_2 (g)$, if rate = $k [\text{H}_2\text{O}_2]$
$2\text{H}_2\text{O}_2 (l) \rightarrow 2\text{H}_2\text{O} (l) + \text{O}_2 (g)$, if rate = $k [\text{H}_2\text{O}_2]$
- A$0$
- Correct answerB$1$
- C$2$
- D$3$
Solution
The rate law for the given reaction is provided as rate = $k [\text{H}_2\text{O}_2]$.
The order of a reaction is defined as the sum of the exponents of the concentration terms in the rate law expression.
In this rate law, the exponent of the concentration of $\text{H}_2\text{O}_2$ is $1$.
Therefore, the order of the reaction is $1$.
Answer: $1$
The order of a reaction is defined as the sum of the exponents of the concentration terms in the rate law expression.
In this rate law, the exponent of the concentration of $\text{H}_2\text{O}_2$ is $1$.
Therefore, the order of the reaction is $1$.
Answer: $1$
Hence, the correct answer is option: 'B'.