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What is the lot of energy (J or Wh) essential to boil one litre the tap-water in a continual kettle starting at room temperature (20°C)?

The calculation chin assuming ideal and standard prerequisites would be interesting as well as factoring in the non-purity of tap-water and also a usual kettle power factor.

It is simple. Density of water is $1\;\frac\textg\textml$ together we have 1 kg water.

Now according to the legislations of calorimetry the amount of heat required

$Q = c \cdot m \cdot \left( 100\text ^\circ\textC - T \right) + \Delta h_\textvap \cdot m$

Here

$c$ = certain heat volume of water, which is 1 cal/(g °C)$m$ = fixed of water; i.e. 1 kg$T$ = the room temperature in °C

So friend will obtain the lot of power needed (in cal) to boil a litre of water

To gain answer in Joule main point the answer in cal by 4.184 J/cal. And be mindful with units!

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edited Mar 17 "17 at 20:10

LShaver
answered Mar 14 "15 at 13:25

Chinmay ChandakChinmay Chandak
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