If the instantaneous rate of reaction is stated as $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$,identify the reaction.

Consider the elementary reaction $A_{(g)} + B_{(g)} \rightarrow C_{(g)} + D_{(g)}$. If the volume of the reaction mixture is suddenly reduced to $\frac{1}{3}$ of its initial volume,the reaction rate will become '$x$' times the original reaction rate. The value of $x$ is:

Select the correct reaction for the given rate: $\text{rate} = -\frac{1}{6} \frac{d[A]}{dt} = -\frac{1}{4} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} = \frac{1}{4} \frac{d[D]}{dt}$

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

For the reaction $2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ s^{-1}$. What is the rate of disappearance of $B$?

For the reaction $3A \to 2B$,the rate of reaction is expressed as $\frac{+d[B]}{dt} = \dots$