MCQ
The general formula for monocarboxylic acids is
- A${C_n}{H_n}COOH$
- B${C_n}{H_{2n + 1}}COOH$
- C${C_n}{H_{2n}}{O_2}$
- ✓Both $(b)$ and $(c)$
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| Rate constant | Activation energy | |
| Step $1$ | $k_1$ | $E_{a_1} = 180\,kJ /mol$ |
| Step $2$ | $k_2$ | $E_{a_2} = 80\,kJ /mol$ |
| Step $3$ | $k_3$ | $E_{a_3} = 50\,kJ /mol$ |
overall rate constant, $k = {\left( {\frac{{{k_1}{k_2}}}{{{k_3}}}} \right)^{2/3}}$ overall activation energy of the reaction will be ........ $kJ\,mol$
Type of reaction in above reaction is
$STATEMENT-2$: The $\mathrm{Fe}$ in $\left[\mathrm{Fe}\left(\mathrm{H}_2 \mathrm{O}\right)_5 \mathrm{NO}_3 \mathrm{SO}_4\right.$ has three unpaired electrons.
$\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}(\mathrm{aq}), \mathrm{Ka}=1.2 \times 10^{-5}$
$\left[\mathrm{K}_{\mathrm{n}}:\right.$ dissociation constant]
The osmotic pressure of $0.03 \mathrm{M}$ aqueous solution of $\mathrm{HX}$ at $300 \mathrm{~K}$ is ............... $\times 10^{-2}$ bar (nearest integer).
$\left[\right.$ Given : $\mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{Mol}^{-1} \mathrm{~K}^{-1}$ ]