Consider the reaction,$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$. In the figure below,identify the curves $X, Y$ and $Z$ associated with the three species in the reaction.

In a catalytic conversion of $N_2$ to $NH_3$ by Haber's process,the rate of reaction was expressed as change in the concentration of ammonia per time is $40 \times 10^{-3} \ mol \ L^{-1} s^{-1}$. If there are no side reactions,the rate of the reaction as expressed in terms of hydrogen is (in $mol \ L^{-1} s^{-1}$)

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

The term $\left( -\frac{dc}{dt} \right)$ in a rate equation refers to the:

In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is:

Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are: