(Solved): A \( 25.0-\mathrm{g} \) sample of copper at \( 90.0^{\circ} \mathrm{C} \) is placed in \( 100.0 \m ...

A \( 25.0-\mathrm{g} \) sample of copper at \( 90.0^{\circ} \mathrm{C} \) is placed in \( 100.0 \mathrm{~g} \) of water at \( 20.0^{\circ} \mathrm{C} \). The copper and water quickly come to the same temperature by the process of heat transfer from copper to water. Calculate the final temperature of the water. Assume that the molar heat capacity of water and copper are \( 75.2 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \) and 24.5 \( \mathrm{J} \mathrm{K}^{-1} \mathrm{~mol}^{-1} \) respectively.