A 82.46 gram copper metal is heated to 138.5°C and dropped into 110.48 gram of water at an initial temperature of Tw. When equilibrium is reached the temperature of copper-water mixture is 25°C. Calculate the initial temperature of water? If the specific heat of copper is 385 J/kg°C and Specific heat of water is 4186 J/kg°C. Initial temperature of water in (°C) =

314.0 kg copper bar is put into a smelter for melting. The initial temperature of the copper is 299.0 K. How much heat in kilojoules must the smelter produce to completely melt the copper bar? (The specific heat for copper is 386 J/kg•K, the heat of fusion for copper is 205 kJ/kg, and its melting point is 1357 K.)

Two 39.5-g ice cubes initially at 0°C are added to 460 g of water at 22.0°C. Assuming this system is insulated and ignoring heat transfer with the glass, what is the equilibrium temperature of the mixture? °C

An aluminum cup with mass 0.56 kg holds 0.96 kg of water. Both the cup and the water have a temperature of 10.°C. If a 0.76-kg piece of copper at 53.°C is added to the cup, what is the final equilibrium temperature in °C? You may assume that the cup, water, and copper are well insulated from anything else.

11.4 kg sample of water at 8°C is in a calorimeter. You drop a piece of iron with a mass of 0.41 kg at 215°C into it. After the sizzling subsides, what is the final equilibrium temperature?    (Given: Sp. Heat of water 1cal/g°C & Sp. Heat of iron is 0.106 cal/g°C) a) Equilibrium temperature in celcius=?

Problem 2: 0.4 kg of ice at – 10°C are mixed with 0.2 kg of water at 50°C. The water and ice are mixed in a calorimeter so that no heat escapes the system. The specific heat of ice is c; = 2090 J/(kg.°C), the la- tent heat of fusion of water is Lf = 3.33× 10° J/kg, and the specific heat of water is cu = 4186 J/(kg-°C). (a) What is the final temperature of the system? (b) How many kg of ice remain in the end? (c) How many kg of water remain in the end?