For the reaction $4KClO_3 \to 3KClO_4 + KCl$,if $-d[KClO_3]/dt = K_1[KClO_3]^4$,$d[KClO_4]/dt = K_2[KClO_3]^4$,and $d[KCl]/dt = K_3[KClO_3]^4$,then:

In the contact process for the manufacture of sulfur trioxide,the reaction is $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$. If the rate of reaction is given by $-\frac{d[O_2]}{dt} = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$,what is the rate of disappearance of $SO_2$?

For the reaction $\frac{1}{2} A \rightarrow 2B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by which of the following expressions?

In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

The average rate of reaction $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$ is written as

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$. The rate of consumption of $H_2$ under the same condition is $..... \ kg \ L^{-1} \ h^{-1}$.