For a reaction of the type $\mathrm{A}+\mathrm{B}\to \mathrm{X}$ products, it is observed that doubling the concentration of $\mathrm{A}$ causes the reaction rate $\left({\mathrm{k}}_1\right)$ to be four-times as great, but doubling the amount of $\mathrm{B}$ does not affect the rate $\left({\mathrm{k}}_2\right)$. The rate equation is

$\mathrm{A}+{\mathrm{B}}_2\rightleftharpoons \mathrm{AB}+\mathrm{B}\dots \dots .\mathrm{ }{\mathrm{k}}_1$

$\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{AB}\dots ....\mathrm{ }{\mathrm{k}}_2$

Consider the following reactions
$\mathrm{A}\to \mathrm{P}1;\mathrm{B}\to \mathrm{P}2;\mathrm{C}\to \mathrm{P}3;\mathrm{D}\to \mathrm{P}4$
The order of the above reactions are $\mathrm{a}, \mathrm{b}, \mathrm{c} \mathrm{and} \mathrm{d},$respectively. The following graph is obtained when log[rate] vs.log[conc.] are plotted:

  
Among the following, the correct sequence for the order of the reactions is :

For an elementary chemical reaction, ${\mathrm{A}}_2 \underset{{\mathrm{k}}_{-1}}{\overset{{\mathrm{k}}_1}{\rightleftarrows }}2\mathrm{A}$ , the expression for $\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}$ is:

Which of the following expression is correct for the rate of reaction given below ?

$5{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)+{\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right)+6{\mathrm{H}}^{+}\left(\mathrm{aq}\right)⟶3{\mathrm{Br}}_2\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

The results given in the below table were obtained during kinetic studies of the following reaction: $2\mathrm{A}+\mathrm{B}\to \mathrm{C}+\mathrm{D}$

X and Y in the given table are respectively :

In the following reaction; $\mathrm{x}\mathrm{A}\to \mathrm{y}\mathrm{B}$

${\log }_{10}\left[-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{d}\mathrm{t}}\right]={\log }_{10}\left[-\frac{\mathrm{d}\left[\mathrm{B}\right]}{\mathrm{d}\mathrm{t}}\right]+0.3010$

‘A’ and ‘B’ respectively can be: