Problem: A 27.5 g aluminum block is warmed to 65.0°C and plunged into an insulated beaker containing 55.1 g water initially at 22.4°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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- qAl = qH2O-(mcT)Al =(mcT)H2O


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Problem Details

A 27.5 g aluminum block is warmed to 65.0°C and plunged into an insulated beaker containing 55.1 g water initially at 22.4°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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