Difficult
What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
(N/A) Molecularity 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.
$1.$ For the reaction $NH_4NO_2 \rightarrow N_2 + 2H_2O$,only one molecule of $NH_4NO_2$ is involved. Thus,it is a unimolecular reaction (molecularity = $1$).
$2.$ For the reaction $2HI \rightarrow H_2 + I_2$,two molecules of $HI$ are involved. Thus,it is a bimolecular reaction (molecularity = $2$).
$3.$ For the reaction $2NO + O_2 \rightarrow 2NO_2$,three molecules ($2$ of $NO$ and $1$ of $O_2$) are involved. Thus,it is a termolecular reaction (molecularity = $3$).
$1.$ For the reaction $NH_4NO_2 \rightarrow N_2 + 2H_2O$,only one molecule of $NH_4NO_2$ is involved. Thus,it is a unimolecular reaction (molecularity = $1$).
$2.$ For the reaction $2HI \rightarrow H_2 + I_2$,two molecules of $HI$ are involved. Thus,it is a bimolecular reaction (molecularity = $2$).
$3.$ For the reaction $2NO + O_2 \rightarrow 2NO_2$,three molecules ($2$ of $NO$ and $1$ of $O_2$) are involved. Thus,it is a termolecular reaction (molecularity = $3$).
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Similar Questions
What is the molecularity and order of the following reaction if the rate law is $\text{rate} = k[O_3][O]$ respectively?
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
$1 \ L$ of $2 \ M$ $CH_3COOH$ is mixed with $1 \ L$ of $3 \ M$ $C_2H_5OH$ to form an ester. The rate of the reaction with respect to the initial rate when each solution is diluted with an equal volume of water will be (in times).
DifficultKCET 2019
View SolutionThe reaction $CH_{3}COF + H_{2}O \rightleftharpoons CH_{3}COOH + HF$ is studied under two conditions:
Condition $I$: $[H_{2}O]_{0} = 1.00 \ M$,$[CH_{3}COF]_{0} = 0.01 \ M$
Condition $II$: $[H_{2}O]_{0} = 0.02 \ M$,$[CH_{3}COF]_{0} = 0.80 \ M$
Time $(t)$ min (Condition $I$) / $[CH_{3}COF]$ $M$ Time $(t)$ min (Condition $II$) / $[H_{2}O]$ $M$ $0$ / $0.01000$ $0$ / $0.0200$ $10$ / $0.00867$ $10$ / $0.0176$ $20$ / $0.00735$ $20$ / $0.0156$ $40$ / $0.00540$ $40$ / $0.0122$
Determine the overall order of the reaction and calculate the rate constant.
Condition $I$: $[H_{2}O]_{0} = 1.00 \ M$,$[CH_{3}COF]_{0} = 0.01 \ M$
Condition $II$: $[H_{2}O]_{0} = 0.02 \ M$,$[CH_{3}COF]_{0} = 0.80 \ M$
| Time $(t)$ min (Condition $I$) / $[CH_{3}COF]$ $M$ | Time $(t)$ min (Condition $II$) / $[H_{2}O]$ $M$ |
|---|---|
| $0$ / $0.01000$ | $0$ / $0.0200$ |
| $10$ / $0.00867$ | $10$ / $0.0176$ |
| $20$ / $0.00735$ | $20$ / $0.0156$ |
| $40$ / $0.00540$ | $40$ / $0.0122$ |
Determine the overall order of the reaction and calculate the rate constant.
The velocity constant of a reaction is $K$. Which of the following statements is not true regarding $K$?
Medium
View SolutionHow can you determine the rate law of the following reaction?
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$
Easy
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