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Enthalpy

36 ml of pure...

Question

36 ml of pure water takes 100 sec to evaporate from a vessel and heater connected to an electric source which delivers 806 watts. The ${Δ H}_{v a p o r i z a t i o n}$ of $H_{2} O$ is:

40.3 k J / m o l

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43.2 k J / m o l

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4.03 k J / m o l

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None of these

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Solution

The correct option is B $40.3 k J / m o l$
Volume of water $= 36 m l$
We know
$D e n s i t y = \frac{M a s s}{V o l u m e}$
Density of water $= 1 g m / m l$
$M a s s = 36 g m$
$M o l e s = \frac{M a s s}{M o l a r m a s s}$
Molar mass of water $= 2 m o l$
Now,
$E n e r g y = P o w e r \times t i m e$
$= 806 \times 100$
$= 80600 J = 80.6 k J$
For $2 m o l$ energy $= 80.6 k J$
For $1 m o l$ energy $= \frac{80.6}{2} = 40.3 K J / m o l$

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