A 1.50kg lump of aluminium [c]at 100, degrees is dropped into a beaker containing 1.00kg of water at 20.0 ∘C. The specific heat capacity of pure water is 4200J/(kg ∘C).
Assuming the system is well insulated, what temperature will the aluminium and water be at thermal equilibrium?
A 1.50kg lump of aluminium [c]at 100, degrees is dropped into a beaker containing 1.00kg of water at 20.0 ∘C. The specific heat capacity of pure water is 4200J/(kg ∘C).
Assuming the system is well insulated, what temperature will the aluminium and water be at thermal equilibrium?
Why are you not posting this in the physics forum?
The final temperature of both the aluminium and the water will be the same (that's the question). You know the energy change in the aluminium must equal the energy change in the water. Can you see how to proceed?
Why are you not posting this in the physics forum?
The final temperature of both the aluminium and the water will be the same (that's the question). You know the energy change in the aluminium must equal the energy change in the water. Can you see how to proceed?
A 1.50kg lump of aluminium [c]at 100, degrees is dropped into a beaker containing 1.00kg of water at 20.0 ∘C. The specific heat capacity of pure water is 4200J/(kg ∘C).
Assuming the system is well insulated, what temperature will the aluminium and water be at thermal equilibrium?
you do a subject as mind-boggling as physics, big respect to you.