A hot lump of 37.4 g of aluminum at an initial temperature of 65.9 °C is placed in 50.0 mL H,O initially at 25.0 C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g.°C)? Assume no heat is lost to surroundings. Trinal °C

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A hot lump of 37.4 g of aluminum at an initial temperature of 65.9 °C is placed in 50.0 mL H,O initially at 25.0 °C and allowed
to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum
is 0.903 J/(g.°C)? Assume no heat is lost to surroundings.
Trinal
°C
Transcribed Image Text:A hot lump of 37.4 g of aluminum at an initial temperature of 65.9 °C is placed in 50.0 mL H,O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g.°C)? Assume no heat is lost to surroundings. Trinal °C
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