For the reaction H_{2(g)} + Br_{2(g)} to 2HBr | vedclass

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Question

(A) The molecularity of a reaction is defined as the number of reacting species (atoms,ions,or molecules) taking part in an elementary reaction,which

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$2, \frac{3}{2}$

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(A) The molecularity of a reaction is defined as the number of reacting species (atoms,ions,or molecules) taking part in an elementary reaction,which must collide simultaneously in order to bring about a chemical reaction.For the given reaction $H_{2(g)} + Br_{2(g)} 	o 2HBr_{(g)}$,the stoichiometric coefficients indicate that $1$ molecule of $H_2$ and $1$ molecule of $Br_2$ are involved,so the molecularity is $1 + 1 = 2$.The order of reaction is the sum of the powers of the concentration terms in the rate law expression.Given $	ext{rate} = K[H_2]^1[Br_2]^{1/2}$,the order is $1 + \frac{1}{2} = \frac{3}{2}$.Therefore,the molecularity is $2$ and the order is $\frac{3}{2}$.

For the reaction $H_{2(g)} + Br_{2(g)} \to 2HBr_{(g)}$,the experimental data suggest,$\text{rate} = K[H_2][Br_2]^{1/2}$. The molecularity and order of the reaction are respectively:

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