The following data are for the decomposition of ammonium nitrate in aqueous solution Volume of ....... The order of the reaction is

${N_2}$ in $cc$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$
Time (minutes)	$10$	$15$	$20$	$25$	Finally

Reaction rate between two substance $A$ and $B$ is expressed as following $:$ rate $= k[A ]^n[B]^m$ If the concentration of $A$ is doubled and concentration of $B$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

From the following which is a second order reaction

For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -

Step$-1$ : ${\text{A  +  E }} \rightleftharpoons AE$ (fast)

Step$-2$ :${\text{AE  +  A }} \to {A_2} + E$ (slow)

Step$-3$ :${{\text{A}}_2}{\text{ +  B }} \to {\text{D}}$ (fast)

what rate law best agrees with this mechanism