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11 Dec 2019
A hot lump of 42.0 g of aluminum at an initial temperature of 59.6 °C is placed in 50.0 mL of H2O 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.
A hot lump of 42.0 g of aluminum at an initial temperature of 59.6 °C is placed in 50.0 mL of H2O 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.
Nelly StrackeLv2
13 Dec 2019