Medium
From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant: $(iv) \ C_{2}H_{5}Cl_{(g)} \rightarrow C_{2}H_{4(g)} + HCl_{(g)} \quad \text{Rate} = k[C_{2}H_{5}Cl]$
(A) Given rate expression is $\text{Rate} = k[C_{2}H_{5}Cl]^1$.
Since the exponent of the concentration term $[C_{2}H_{5}Cl]$ is $1$,the order of the reaction is $1$.
The dimension of the rate constant $k$ is calculated as:
$k = \frac{\text{Rate}}{[C_{2}H_{5}Cl]} = \frac{\text{mol} \ L^{-1} \ s^{-1}}{\text{mol} \ L^{-1}} = s^{-1}$.
Since the exponent of the concentration term $[C_{2}H_{5}Cl]$ is $1$,the order of the reaction is $1$.
The dimension of the rate constant $k$ is calculated as:
$k = \frac{\text{Rate}}{[C_{2}H_{5}Cl]} = \frac{\text{mol} \ L^{-1} \ s^{-1}}{\text{mol} \ L^{-1}} = s^{-1}$.
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Similar Questions
What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
Difficult
View SolutionThe rate constant of a first order reaction at $27^{\circ} C$ is $10^{-3} \ min^{-1}$. The temperature coefficient of this reaction is $2$. What is the rate constant (in $min^{-1}$) at $17^{\circ} C$ for this reaction?
The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are:
DifficultAIPMT 2011
View Solution$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?
The mechanism for the reaction is given below:
$2P + Q \to S + T$
$P + Q \to R + S$ (slow)
$P + R \to T$ (fast)
The rate law expression for the reaction is:
$2P + Q \to S + T$
$P + Q \to R + S$ (slow)
$P + R \to T$ (fast)
The rate law expression for the reaction is:
Medium
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