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500 g of water is heated from 30^(@)C to...

500 g of water is heated from `30^(@)C` to `60^(@)C`. Ignoring the slight expansion of water, calculate the change in internal energy of the water ? (Specific heat of water 4184 J/kg.K)

Text Solution

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When the water is heated from `30^(@)C` to `60^(@)C`, there is only a slight change in its volume. So we can treat this process as isochoric. In an isochoric process the work done by the system is zero. The given heat supplied is used to increase only the internal energy.
`DeltaU=Q=ms_(V)DeltaT`
The mass of water=`500g=0.5kg`
The change in temperature=30K
The heat `Q=0.5xx4184xx30=62.76kJ`
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