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Derive the relationship between rate of reaction, rate of disappearance of $X, Y$ and rate of formation of $X_{2} Y_{2}$ for the reaction :$$2 X+3 Y \longrightarrow X_{2} Y_{3}$$
The reaction; $2 \mathrm{~N}_{2} \mathrm{O}_{5} \longrightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$, shows an increase inconcentration of $\mathrm{NO}_{2}$ by $20 \times 10^{-3}$ mol litre $^{-1}$ in 5 second. Calculate(a) rate of appearance of $\mathrm{NO}_{2}$,(b) rate of reaction and(c) rate of disappearance of $\mathrm{N}_{2} \mathrm{O}_{5}$.
From the rate expression for the following reactions, determine their order of renction and the dimensions of the rate constants.(u) $\mathrm{WNO}_{(\mathrm{k})} \cdots \mathrm{N}_{2} \mathrm{O}_{(\mathrm{g})}+\mathrm{NO}_{2(\mathrm{~g})} ; \quad$ Rate $=K[\mathrm{NO}]^{2}$Rate $=K\left[\mathrm{H}_{2} \mathrm{O}_{2}\right][\mathrm{I}]$(c) $\mathrm{CH}_{3} \mathrm{CHO}_{(\mathrm{g})} \longrightarrow \mathrm{CH}_{4(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} ;$ Rate $=K\left[\mathrm{CH}_{3} \mathrm{CHO}\right]^{3 / 2}$(d) $\mathrm{CHCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(g)} \longrightarrow \mathrm{CCl}_{4(\mathrm{~g})}+\mathrm{HCl}_{(\mathrm{g})}$Rate $=K\left[\mathrm{CHCl}_{3}\right]\left[\mathrm{Cl}_{2}\right]^{1 / 2}$
For; $\begin{gathered}2 A+B+C \longrightarrow \text { Products, calculate the; } \\ \text { (excess): }\end{gathered}+B+C \longrightarrow \longrightarrow \longrightarrow$(a) rate expression.(b) units of rate and rate constant.(c) effect on rate if concentration of $A$ is doubled and of $B$ is tripled.
At $25^{\circ} \mathrm{C}$, the rate constant for the reaction $\Gamma+\mathrm{ClO}^{-} \longrightarrow \mathrm{IO}^{-}+\mathrm{Cl}^{-}$is $0.0606$ litre $\mathrm{mol}^{-1} \mathrm{sec}^{-1}$. If a solution is initially $1.0 \mathrm{M}$. in $\mathrm{I}$ and $5.0 \times 10^{-4} \mathrm{M}$ in $\mathrm{ClO}^{-}$. Can you calculate the $\left[\mathrm{ClO}^{-}\right]$ after $300 \mathrm{sec}$. If yes, then how much. If no, then why?
