MCQ
A solution of $1 $ molal concentration of a solute will have maximum boiling point elevation when the solvent is
- AEthyl alcohol
- BAcetone
- ✓Benzene
- DChloroform
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$\mathrm{HX}(\mathrm{aq}) \rightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{X}(\mathrm{aq}), \mathrm{Ka}=1.2 \times 10^{-5}$
$\left[\mathrm{K}_{\mathrm{n}}:\right.$ 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 : $\mathrm{R}=0.083 \mathrm{~L} \mathrm{bar} \mathrm{Mol}^{-1} \mathrm{~K}^{-1}$ ]
$\operatorname{P}t|{{H}_{{{2}_{\left( 2\,atm \right)}}}}|H_{\left( 0.02\,M \right)}^{\oplus }||H_{\left( 0.1\,M \right)}^{\oplus }|{{H}_{{{2}_{\left( 1\,atm \right)}}}}|Pt$
$\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$
$\text { rate }=\mathrm{k}[\mathrm{A}]^{1 / 2}[\mathrm{~B}]^{1 / 2}$
The reaction is initiated by taking $1 \mathrm{M}$ concentration $A$ and $B$ each. If the rate constant $(k)$ is $4.6 \times 10^{-2} \mathrm{~s}^{-1}$, then the time taken for $\mathrm{A}$ to become $0.1 \mathrm{M}$ is . . . . . . . . . . sec. (nearest integer)
Statements $I$ : $SbCI _5$ is more covalent than $SbCI _3$
Statements $II$: The higher oxides of halogens also tend to be more stable than the lower ones.
In the light of the above statements, choose the most appropriate answer from the options given below
Product $(A)$ of above reaction will be