Question

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 = \(k[\text{H}_2\text{O}_2]\)

• A. \(0\)
• B. \(1\)
• C. \(2\)
• D. \(3\)

Hint:

The order is the sum of the powers of concentration terms in the rate law.

Answer 1

The Correct Option is B

Step 1: Use the definition:
Order = sum of exponents in the rate expression.

Step 2: Read the exponent:
Only one concentration term appears, $[\text{H}_2\text{O}_2]$, and no exponent is written, so it is 1.

Step 3: Conclude:
Order = 1, option B. The decomposition of hydrogen peroxide is a well-known first-order reaction.

Final Answer:
The only exponent in the rate law is 1, so the order is 1. \[ \boxed{\text{(B) }1} \]