$45 g$ of water at $50^{\circ} C$ in a beaker is cooled when $50 g$ of copper at $18^{\circ} C$ is added to it. The contents are stirred till a final constant temperature is reached. Calculate this final temperature. The specific heat capacity of copper is $40.39 J g^{- 1} K^{- 1}$ and that of water is $4.2 J g^{- 1} K^{- 1}$ .

17^{\circ} C

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27^{\circ} C

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47^{\circ} C

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none of the above

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Solution

The correct option is D $47^{\circ} C$
The final temperature is given as $\frac{m_{1} c_{1} t_{1} + m_{2} c_{2} t_{2}}{m_{1} c_{1} + m_{2} c_{2}} = \frac{45 \times 50 \times 4.2 + 50 \times 18 \times 0.39}{45 \times 4.2 + 50 \times 0.39} = 9801 / 208.5 = 47^{o} C$

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Similar questions

45 g

of water at

50^{o} C

in a breaker is cooled when

50 g

of copper at

18^{o} C

is added to it. The contents are stirred till a final constant temperature is reached. Calculate this final temperature. The specific heat capacity of copper is

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

and that of water is

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

. State the assumption used

45 g

of water at

50^{\circ} C

in a beaker is cooled when

50 g

of copper at

18^{\circ} C

is added to it. The contents are stirred till final constant temperature is reached. Calculate the final temperature. The specific heat capacity of copper is

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

and that of water is

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

. State the assumption used.

A mass of 50 g of a certain metal at $150^{\circ} C$ is immersed in 100 g of water at $11^{\circ} C$ . The final temperature is $20^{\circ} C$ . Calculate the specific heat capacity of the metal. Assume that the specific heat capacity of water is 4.2 J $g^{- 1} K^{- 1}$ .