5) A calorimeter contains 25.00 g water at 23.8 degrees celsius. A 5.00 g hot metal at 78.3 degrees celsius dropped into the calorimeter. Calculate the specific heat of the unknown metal if the final tempertature of mixture is found to be 46.4 degrees celsius.
6) Consider a mixture of 75.0 g water at room temperature 23.0 degrees celsius and 25.0 g water at 95.0 degrees celsius. Calculate the equilibrium temperature of the mixture.
Answer:
q ( H2O ) = 25.00 g x 4.18 J/ g°C ( 46.4 - 23.8 ) = 2362 J
q ( metal ) = - 2362 J
- 2362 = 5.00 x specific heat x ( 46.4 - 78.3 )
- 2362 = - 1595 x specific heat
specific heat = 14.8 J/ g°C
(75.0 x 23) + (25.0 x 95.0) = (75.0+25.0) T
T = 41 °C
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