The rate law for the reaction, $x \mathrm{~A}+y \mathrm{~B} \longrightarrow \mathrm{mP}+\mathrm{nQ}$, is $\mathrm{r}=\mathrm{k}[\mathrm{A}]^{\mathrm{c}} \times[\mathrm{B}]^{\mathrm{d}}$ What is the overall order of reaction?
$(x+y)$
$(m+n)$
$(\mathrm{c}+\mathrm{d})$
$\frac{x}{y}$
Calculate the molal elevation constant of water if boiling point of 0.7 m solution of non volatile solute is 373.5 K .
[Boiling point of water $=373.15 \mathrm{~K}$ ]
$0.4 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$
$0.25 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$
$0.5 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$
$0.60 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$
Calculate the work done in following reaction.
$$ \begin{aligned} & \mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{HCl}_{(\mathrm{g})} \longrightarrow \mathrm{C}_2 \mathrm{H}_5 \mathrm{Cl}_{(\mathrm{g})} \text { at } 27^{\circ} \mathrm{C} . \\ & \left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right) \end{aligned} $$
$\quad 4988.4 \mathrm{~J}$
$\quad-1247.1 \mathrm{~J}$
2494.2 J
3741.3 J
At 298 K pH of a solution is 13 . What is the number of $\mathrm{H}_3 \mathrm{O}^{+}$ions present in one mL of this solution?
$6.022 \times 10^7$
$5.020 \times 10^8$
$7.022 \times 10^{13}$
$1 \times 10^{13}$
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