A 43.5-g sample of copper at 99.9 °C is dropped into a beaker containing 156 g of water at 18.7 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g ⋅ K and 0.385 J/g ⋅ K, respectively.)

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A 43.5-g sample of copper at 99.9 °C is dropped into a beaker containing 156 g of water at 18.7 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g ⋅ K and 0.385 J/g ⋅ K, respectively.)

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