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?

Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$

Which statement about the above equation is wrong?

Following is the rate constant of reaction what is the overall order of reaction ?

$(a)$ $6.66 \times 10^{-3} \,s ^{-1}$

$(b)$ $4.5 \times 10^{-2} \,mol ^{-1} \,L \,s ^{-1}$

The rate of certain reaction depends on concentration according to the equation $\frac{{ - dc}}{{dt}}\, = \,\frac{{{K_1}C}}{{1 + {K_2}C}},$ what is the order, when concentration $(c)$ is very-very high

The reaction $2 NO + Br _2 \rightarrow 2 NOBr$

takes places through the mechanism given below :

$NO + Br _2 \Leftrightarrow NOBr _2 \text { (fast) }$

$NOBr _2+ NO \rightarrow 2 NOBr \text { (slow) }$

The overall order of the reaction is $.....$.

The elementary reaction $2SO_2(g) + O_2(g) \to 2SO_3(g)$ is carried out in $1\, dm^3$ vessel and $2\,dm^3$ vessel separately. The ratio of the reaction velocities will be