Consider the reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$. The equality relationship between $\frac{d[NH_3]}{dt}$ and $\frac{d[H_2]}{dt}$ is

For the reaction,$XA + YB \rightarrow ZC$,if $\frac{- d [ A ]}{ dt } = \frac{- d [ B ]}{ dt } = \frac{d [ C ]}{ dt },$ then the correct statement among the following is:

In a reaction,$n_1A + n_2B \to m_1C + m_2D$,$5 \ M$ of reactant $A$ are allowed to react with $3 \ M$ of reactant $B$. After $5 \ sec$,the concentration of $A$ was found to be $4 \ M$. What are the rate of decomposition of $A$ and the rate of formation of $D$,respectively?

Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?

$NO_2$ required for a reaction is produced by decomposition of $N_2 O_5$ in $CCl_4$ as per the equation $2 \, N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$. The initial concentration of $N_2 O_5$ is $3 \, mol \, L^{-1}$ and it is $2.75 \, mol \, L^{-1}$ after $30 \, minutes$. The rate of formation of $NO_2$ is $x \times 10^{-3} \, mol \, L^{-1} \, min^{-1}$. The value of $x$ is . . . . . . .

$A \rightarrow P$ is a first order reaction. The following graph is obtained for this reaction,($x$-axis $=$ time; $y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is