A 46.2 g sample of copper is heated to 95.4°C and then placed in a calorimeter containing 75.0 g water at 19.6°C. The final temperature of the metal and water is 21.8°C. Calculate the specific heat capacity of copper, assuming that all the heat lost by the copper is gained by the water.
Note: Please double check the number of significant figures.
_________J/g·°C
A 46.2 g sample of copper is heated to 95.4°C and then placed in a calorimeter containing 75.0 g water at 19.6
46.2 ( 21.8 - 95.4 ) x specific heat =
= - 75 ( 21.8 - 19.6 ) x 4.186
- 3400 x specific heat = -690.69
specific heat copper = 0.203 J/g°C
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