$(1)$ $\left[\mathrm{Co}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}$ $\quad\quad\quad1$ chelate ring
$(2)$ $\left[\mathrm{Co}(\mathrm{en})_{3}\right] \mathrm{Cl}_{2}$ $\quad\quad\quad\quad\quad\quad3$ chelate ring
$(3)$ $\left[\mathrm{Co}(\mathrm{en})_{2}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{Cl}_{2}$ $\quad\quad\quad2$ chelate ring
$(4)$ $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2} \quad\quad\quad\quad\quad0$ chelate ring
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In the above first order reaction the concentration of $\mathrm{PCl}_{5}$ reduces from initial concentration $50\, mol\,\mathrm{L}^{-1}$ to $10\, \mathrm{~mol} \,\mathrm{~L}^{-1}$ in $120\, minutes$ at $300\, \mathrm{~K}$. The rate constant for the reaction at $300\, \mathrm{~K}$ is $\mathrm{X}$ $\times 10^{-2} \mathrm{~min}^{-1}$. The value of $x$ is $......$
$[$ Given $\log 5=0.6989]$
$CH_3COCH_{3(aq)} + Br_{2(aq)} \rightarrow $$CH_3COCH_2Br_{(aq)} + H^+_{(aq)}+ Br^-_{(aq)}$
These kinetic data were obtained for given reaction concentrations.
Initial concentrations, $M$
| $[CH_3COCH_3]$ | $[Br_2]$ | $[H^+]$ |
| $0.30$ | $0.05$ | $0.05$ |
| $0.30$ | $0.10$ | $0.05$ |
| $0.30$ | $0.10$ | $0.10$ |
| $0.40$ | $0.05$ | $0.20$ |
Initial rate, disappearance of $Br_2, \,\,Ms^{-1}$
$5.7 \times 10^{-5} ,$ $5.7 \times 10^{-5} ,$ $1.2 \times 10^{-5} ,$ $3.1 \times 10^{-5}$
Based on these data, the rate equation is