The decomposition of dimethyl ether leads to the formation of $CH _{4}, H _{2}$ and $CO$ and the reaction rate is given by
Rate $=k\left[ CH _{3} OCH _{3}\right]^{3 / 2}$
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.
Rate $=k\left(p_{ CH _{3} OCH _{3}}\right)^{3 / 2}$
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
The decomposition of dimethyl ether leads to the formation of $CH _{4}, H _{2}$ and $CO$ and the reaction rate is given by
Rate $=k\left[ CH _{3} OCH _{3}\right]^{3 / 2}$
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.
Rate $=k\left(p_{ CH _{3} OCH _{3}}\right)^{3 / 2}$
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
If pressure is measured in bar and time in minutes, then
Unit of rate $=$ bar $\min ^{-1}$
Rate $ = k{\left( {{p_{C{H_3}OC{H_3}}}} \right)^{3/2}}$
$ \Rightarrow k = \frac{{{\rm{ Rate }}}}{{{{\left( {{p_{C{H_3}OC{H_3}}}} \right)}^{3/2}}}}$
Therefore, unit of rate constants $(k)=\frac{\text { bar min }^{-1}}{\operatorname{bar}^{3 / 2}}$
$ = ba{r^{ - 1/2}}{\min ^{ - 1}}$
Similar Questions
Explain order of reaction of complex reaction by giving examples.
Explain order of reaction of complex reaction by giving examples.
The rate of the reaction $CC{l_3}CHO + NO \to CHC{l_3} + NO + CO$ is given by Rate $ = K\,[CC{l_3}CHO]\,[NO]$. If concentration is expressed in moles/litre, the units of K are
The rate of the reaction $CC{l_3}CHO + NO \to CHC{l_3} + NO + CO$ is given by Rate $ = K\,[CC{l_3}CHO]\,[NO]$. If concentration is expressed in moles/litre, the units of K are
The rate of reaction $A + 2B \to 3C$ becomes $72\, times$ when concentration of $A$ is tripled and concentration of $B$ is doubled then the order of reaction with respect to $A$ and $B$ respectively is
The rate of reaction $A + 2B \to 3C$ becomes $72\, times$ when concentration of $A$ is tripled and concentration of $B$ is doubled then the order of reaction with respect to $A$ and $B$ respectively is
The rate constant of esterification $(k) = k'\, [H_2O]$ rate constant of esterification $2.0\times 10^{-3}\,min^{-1}$ calculate $k'$.
The rate constant of esterification $(k) = k'\, [H_2O]$ rate constant of esterification $2.0\times 10^{-3}\,min^{-1}$ calculate $k'$.
The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of reaction is -
The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of reaction is -