MCQ
$36\, mL$ of pure water takes $100\, sec$ to evaporate from a vessel and heater connected to an electric source which delivers $806\, watt$. The $\Delta H_{vaporization}$ of $H_2O$ is.....$ kJ/mol$
- ✓$40.3$
- B$43.2$
- C$4.03$
- DNone of these
Total heat supplied for $36\, \mathrm{mL}\, \mathrm{H}_{2} \mathrm{O}$
$=806 \times 100$
$=80600\, \mathrm{J}$
$\Delta \mathrm{H}_{\mathrm{vap}} =\frac{80600}{36} \times 18$
$=40300 \,\mathrm{J} \text { or } 40.3\, \mathrm{kJ} / \mathrm{mol}$
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[Assume : No cyano complex is formed; $K _{ sp }( AgCN )$ $=2.2 \times 10^{-16}$ and $\left. K _{ a }( HCN )=6.2 \times 10^{-10}\right]$