125.0 gram bars of aluminum and copper are heated to 275.6°C in a colorimeter that doesn‘t allow heat to be exchanged with the environment. The two bar are dropped into a colorimeter containing 250.0 gm of water at 10.9°C.What is the final temperature of the water if the specific heat capacity of aluminum and copper are 0.275 calories/gm/°C and 0.385J/gm/‘C respectively? 1 calorie 4.184 joules
Heat mass x heat capacity x temperature change Heat lost by hot aluminium + heat lost by hot copper Heat gained by cold water Let aluminium and copper and water all end at temperature T [125 x 0.275 x (275.6 - T)] + [125 x 0.385/4.184 x (275.6 - T)] [ 250 x 1 x (T - 10.9)] NB 1). use of 4.184 to change J to calories 2). Use of 1 cal/gm/C for heat capacity of water Solving to find T I will leave to you!!! Its math not science/chemistry.
depends did they use water soluble flux.don't worry it will clear up. master plumber
