The rate law expression for the reaction $aA + bB \to P$ is rate $= K [A]^p [B]^q$ The order of the reaction is
The rate law expression for the reaction $aA + bB \to P$ is rate $= K [A]^p [B]^q$ The order of the reaction is
- A
$(a+b)$
- B
$(p+q)$
- C
$(a-b)$
- D
$(p-q)$
Similar Questions
Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$
Which is True $(T)$ and False $(F)$ in the following sentence ?
The reaction is elementary.
Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$
Which is True $(T)$ and False $(F)$ in the following sentence ?
The reaction is elementary.
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 $k'$.
By “the overall order of a reaction”, we mean
By “the overall order of a reaction”, we mean
Select the rate law for reaction $A + B \longrightarrow C$
Exp
$[A]$
$[B]$
Rate
$1$
$0.012$
$0.035$
$0.10$
$2$
$0.024$
$0.070$
$0.80$
$3$
$0.024$
$0.035$
$0.10$
$4$
$0.012$
$0.070$
$0.80$
Select the rate law for reaction $A + B \longrightarrow C$
| Exp | $[A]$ | $[B]$ | Rate |
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.070$ | $0.80$ |
| $3$ | $0.024$ | $0.035$ | $0.10$ |
| $4$ | $0.012$ | $0.070$ | $0.80$ |
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?