Thank you for visiting A 45 5 g sample of copper at 99 8 C was dropped into a beaker containing 152 g of water at 18 5 C. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
Answer :
Final answer:
The final temperature when thermal equilibrium is reached between a copper sample and water can be calculated using the principle of conservation of energy.
Explanation:
The final temperature when thermal equilibrium is reached can be calculated using the principle of conservation of energy. The energy lost by the copper is equal to the energy gained by the water. We can use the equation: (mass of copper)(specific heat of copper)(change in temperature of copper) = (mass of water)(specific heat of water)(change in temperature of water)
Plugging in the values, we get: (45.5 g)(0.39 J/g·°C)(final temperature - 99.8°C) = (152 g)(4.18 J/g·°C)(final temperature - 18.5°C) Solving for the final temperature, we find that it is approximately 20.7°C.
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