In a gaseous reaction 

${A_{2\left( g \right)}} \longrightarrow {B_{\left( g \right)}} + \frac{1}{2}\,{C_{\left( g \right)}}$ the increase in pressure from $100\, mm$ to $120\, mm$ is noticed in $5\,\min$. The rate of dissappearence of $A_2$ in $mm\, min^{-1}$ is

In hydrogenation reaction at ${27\,^o}C$, it is observed that hydrogen gas pressure falls from $2\,atm$ to $1.2\,atm$ in $50\,\min$. Calculate the rate of disappearance of hydrogen

Assertion : The kinetics of the reaction -

$mA + nB + pC \to m' X + n 'Y + p 'Z$

obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.

Reason : The rate of the reaction does not depend upon the concentration of $C$.

For a reaction $A \to$ Products, a plot of $log\,t_{1/2}$ versus $log\,a_0$ is shown in the figure. If the initial concentration of $A$ is represented by $a_0,$ the order of the reaction is

The reaction, $X + 2Y + Z \to  N$ occurs by the following mechanism

$(i)$ $X + Y  \rightleftharpoons  M$             very rapid equilibrium

$(ii)$ $M + Z \to  P$                        slow

$(iii)$ $O + Y \to  N$                       very fast

What is the rate law for this reaction

The hydrolysis of ethyl acetate is a reaction of ......... order

$C{{H}_{3}}COOEt+{{H}_{2}}O\xrightarrow{{{H}^{+}}}C{{H}_{3}}COOH+EtOH$