1
answer
0
watching
114
views
12 Dec 2019
A hot lump of 44.3 g of aluminum at an initial temperature of 85.0 °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 44.3 g of aluminum at an initial temperature of 85.0 °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.
Patrina SchowalterLv2
13 Dec 2019