In the reaction $xA \to yB,$
$0.48 + \log \left\{ -\frac{d[A]}{dt} \right\} = \log \left\{ +\frac{d[B]}{dt} \right\} + 0.7$
Then,$x : y$ is

In a reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \ L^{-1} s^{-1}$):

For the reaction $A + 2B \to C + D$,if $-\frac{d[A]}{dt} = 5 \times 10^{-4} \ mol \ L^{-1} s^{-1}$,then what is the value of $-\frac{d[B]}{dt}$?

For the reaction $3 A + 2 B \rightarrow C$,which statement is correct $:-$

For the reaction $N_{2}O_{5(g)} \rightarrow 2NO_{2(g)} + \frac{1}{2} O_{2(g)}$,the rate of disappearance of $N_{2}O_{5}$ is given as $6.25 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of $NO_{2}$ and $O_{2}$ is given respectively as:

For a general chemical reaction $2A + 3B \rightarrow \text{Products}$,if the rate of disappearance of $A$ is $r_1$ and that of $B$ is $r_2$,then the relationship between $r_1$ and $r_2$ is: