Question:
For the reaction
\(\text{H}_2(g) + \text{Br}_2(g) \to 2 \text{HBr}(g)\),
the experimental data suggest the rate law
\(\text{Rate} = k[\text{H}_2][\text{Br}_2]^{1/2}\).
The molecularity and order of the reaction are respectively
For the reaction
\(\text{H}_2(g) + \text{Br}_2(g) \to 2 \text{HBr}(g)\),
the experimental data suggest the rate law
\(\text{Rate} = k[\text{H}_2][\text{Br}_2]^{1/2}\).
The molecularity and order of the reaction are respectively
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Order comes from rate law, molecularity from reaction equation.
Updated On: Mar 23, 2026
- 2, (3)/(2)
- \(\dfrac{3}{2}, 2\)
- 1, 1
- 1, (1)/(2)
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Verified By Collegedunia
The Correct Option is A
Solution and Explanation
Step 1: Molecularity is number of reacting molecules in the equation = 2.
Step 2: Order of reaction = 1 + (1)/(2) = (3)/(2)
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