•From the problem, we can see that the Copper will be losing heat to the water and the vessel.
•This is because the temperature of the copper is higher than that of the water.
•This means that there will be a thermodynamic equilibrium. And we will use this equation:
A 455-g piece of copper tubing is heated to 89.5°C and placed in an insulated vessel containing 159 g of water at 22.8°C. Assuming no loss of water and a heat capacity of 10.0 J/K for the vessel, what is the final temperature (c of copper = 0.387 J/g·K)?
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.