For the reaction $2A + B \to C$,the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is

$[A] (mol\,L^{-1})$	$[B] (mol\,L^{-1})$	Initial Rate $(mol\, L^{-1}\,s^{-1} )$
$0.05$	$0.05$	$0.045$
$0.10$	$0.05$	$0.090$
$0.20$	$0.10$	$0.72$

 

For reaction $2A + B \to $ products, the active mass of $ B $ is kept constant and that of $A$ is doubled. The rate of reaction will then

An elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?

Write general equation of reaction and explain - what is order of reaction ? Which is its value ?

The rate constant of the reaction $2H_2O_2(aq) \to  2H_2O(aq) + O_2(g)$ is $3\times10^{-3}\, min^{-1}$. At what concentration of $H_2O_2$, the rate of reaction will be $2\times10^{-4}\, M\, s^{-1}$ ? ............ $M$

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?