$200 g$ mass of a certain metal at $83^{\circ} C$ is immersed in $300 g$ of water of $30^{\circ} C$ . Final temperature of combination is $33^{o} C$ .Calculate the specific heat capacity of metal. Assume that the specific heat capacity of water is $4.2 J g^{- 1} K^{- 1}$

0.189 J g^{- 1} K^{- 1}

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0.378 J g^{- 1} K^{- 1}

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3.78 J g^{- 1} K^{- 1}

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0.756 J g^{- 1} K^{- 1}

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Solution

The correct option is B $0.378 J g^{- 1} K^{- 1}$
Specific heat capacity is the amount of heat energy required to change the temperature of unit mass of a substance through $1$ degree centigrade.
Amount of heat lost by metal $=$ amount of heat gained by water
As $H e a t$ $E n e r g y = m s (T_{2} - T_{1})$
$\Rightarrow 200 (s) (83 - 33) = 300 (4.2) (33 - 30)$
$\Rightarrow s = 0.378 J / g K$

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