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A 25.5-g aluminum block is warmed to 65.4C^{\circ} \mathrm{C} and plunged into an insulated beaker containing 55.2 g water initially at 22.2C^{\circ} \mathrm{C}. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?

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Given that a 25.5 Aluminum block initially at 65.4 o^oC is submerged in 55.2 g water initially at 22.2o^oC.

Determine the temperature of both substances assuming that no heat is lost in the process.

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