MCQ
Product $[ X ]$ formed in the above reaction is :


- ✓

- B

- C$H _3 C - CH _2- CH = CH _2$
- D$H _3 C - CH = CH - CH _3$





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$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is
| Column-$I$ | Column-$II$ |
| $(A)$ $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_4\left(\mathrm{H}_2 \mathrm{O}\right)_2\right] \mathrm{Cl}_2$ | $(p)$ geometrical isomers |
| $(B)$ $\left[\mathrm{Pt}\left(\mathrm{NH}_3\right)_2 \mathrm{Cl}_2\right]$ | $(q)$ paramagnetic |
| $(C)$ $\left[\mathrm{Co}\left(\mathrm{H}_2 \mathrm{O}\right)_5 \mathrm{Cl}\right] \mathrm{Cl}$ | $(r)$ diamagnetic |
| $(D)$ $\left[\mathrm{Ni}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_2$ | $(s)$ metal ion with $+2$ oxidation state |
| Expt. No. | $(A)$ | $(B)$ | Initial Rate |
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.070$ | $0.80$ |
| $3$ |
$0.024$ |
$0.035$ | $0.10$ |
| $4$ | $0.012$ | $0.070$ | $0.80$ |
