$200 g$ water is heated from $40^{o} C$ to $60^{o} C$ . Ignoring the slight expansion of water, the change in its internal energy is close to:
(Given specific heat of water $= 4184 J / k g / K$ )

167.4 k J

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16.7 k J

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8.4 k J

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4.2 k J

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Solution

The correct option is A $16.7 k J$
Since expansion is ignored, work done is zero and hence by first law of thermodynamics, internal energy change equals heat supplied.

$Δ U = Q = 0.2 (4184) (20) J = 16.7 k J$

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