In a gaseous reaction $A_{2(g)} \longrightarrow B_{(g)} + \frac{1}{2} C_{(g)}$,the increase in pressure from $100 \text{ mm}$ to $120 \text{ mm}$ is noticed in $5 \text{ min}$. The rate of disappearance of $A_2$ in $\text{mm min}^{-1}$ is

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:

Consider the reaction, $3I^-_{(aq)} + S_2O_8^{2-} (aq) \rightarrow I_3^- (aq) + 2SO_4^{2-} (aq)$. If the rate of formation of $SO_4^{2-}$ at a particular time is $2.2 \times 10^{-2} \text{ mol dm}^{-3} \text{s}^{-1}$, calculate the rate of consumption of $I^-$.

For the reaction $R \to P$,describe the nature of the graphs of $[R]$ versus $time$ and $[P]$ versus $time$.

For the reaction, $3A + 2B \to C + D$, the differential rate law can be written as:

Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is: