What will be the equilibrium temperature when a 277 g block of copper at 322°C is placed in a 175 g aluminum c
Max K:
What will be the equilibrium temperature when a 277 g block of copper at 322°C is placed in a 175 g aluminum calorimeter cup containing 820 g of water at 12.8°C?
What will be the equilibrium temperature when a 277 g block of copper at 322°C is placed in a 175 g aluminum calorimeter cup containing 820 g of water at 12.8°C?
An answer and a explanation would be helpful
I value the explanation over justthe answer
Let the equilibrium temp. be T°c
Mass of copper = mc = 277 gm
Initial tem. of copper = tc = 322°c
Mass of aluminum = ma = 175 gm
Initial temp. of aluminum = ta =12.8°c
Mass of water = mw = 820 gm
Initial temp. of water = tw = 12.8°c
By calorimetry, the heat energy received by (Aluminum + Water) is equal to heat energy given by coper.
The quantity of heat = m x s x t J
277x.385x(322-T) = 175x.897x(T-12.8) + 820×4.2x(T-12.8)
106.645(322-T) = 156.975(T-12.8) + 3444(T-12.8)
34339.69-106.645T=156.975T-2009.28+3444T-44083.2
34339.69+2009.28+44083.2=156.975T+3444T+106.645T
80432.17 = 3707.62 T
T = 80432.17 / 3707.62 = 21.7°c
….. …… ………===================