(B) The reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Since water is present in large excess,its concentration remains effectively constant duri

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Molecularity is $2$ but order of reaction is $1$

(B) The reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Since water is present in large excess,its concentration remains effectively constant during the reaction. Therefore,the rate law is given by $Rate = k[RCl]^1[H_2O]^0 = k'[RCl]^1$. The order of the reaction is the sum of the powers of the concentration terms in the rate law,which is $1 + 0 = 1$. The molecularity is the number of reacting species taking part in an elementary step,which is $2$ ($RCl$ and $H_2O$). Thus,molecularity is $2$ and order is $1$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

In the hydrolysis of an organic chloride in the presence of a large excess of water,the reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Determine the molecularity and order of the reaction.

A
Molecularity and order of reaction both are $2$
B
Molecularity is $2$ but order of reaction is $1$
C
Molecularity is $1$ but order of reaction is $2$
D
Molecularity and order of reaction both are $1$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

If $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)

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The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

Medium

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In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

AIPMT 2012

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For the reaction $3 \, A_{(g)} \xrightarrow{K} B_{(g)} + C_{(g)}$,$K$ is $10^{-14} \, L/mol \cdot min$. If $[A] = 0.5 \, M$,then the value of $-\frac{d[A]}{dt}$ (in $M/sec$) is:

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The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?

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In the hydrolysis of an organic chloride in the presence of a large excess of water,the reaction is $RCl + H_2O \longrightarrow ROH + HCl$. Determine the molecularity and order of the reaction.

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If $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)

The following are the rate constants of two different reactions. What is the overall order of each reaction?$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

For the reaction $3 \, A_{(g)} \xrightarrow{K} B_{(g)} + C_{(g)}$,$K$ is $10^{-14} \, L/mol \cdot min$. If $[A] = 0.5 \, M$,then the value of $-\frac{d[A]}{dt}$ (in $M/sec$) is:

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)$(ii)$ $M + Z \to P$ (slow)$(iii)$ $P + Y \to N$ (very fast)What is the rate law for this reaction?

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The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

The reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?