A jar of tea is placed in sunlight until it reaches an equilibrium temperature of 30.5 •C. In an attempt to cool the liquid, which has a mass of 161 g , 109 g of ice at 0.0 •C is added. At the time at which the temperature of the tea is 24•C, find the mass of the remaining ice in the jar. The specific heat of water is 4186 J/kg · •C. Assume the specific heat capacity of the tea to be that of pure liquid water. Answer in units of g.

A block of metal of mass 0.360 kg is heated to 144.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.170 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). J/(kg · K)

A block of metal of mass 0.280 kg is heated to 148.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.190 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 44.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 x 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). 3/(kg K)

A 1040kg iron bar with a length of 2.00m and temperature of −45.25˚C is immersed in 50kg of liquid water at 90˚C. The specific heat of liquid water 4.186 kJ/(kg˚C), and the latent heat of fusion of water is 333kJ/kg. The specific heat of iron is 0.45kJ/(kg˚C) and its melting point is 1538˚C. The goal is to determine the final temperature of the system (iron+water) once it reaches thermal equilibrium, and also the state of each substance (solid, liquid, gas)   d) If you did (c) correctly, the iron will still be colder than 0˚C, so the system is not yet in thermal equilibrium. As the iron heat up more, the water, already at 0˚C, will cool down. How much mass of water becomes ice?  e) What is the final temperature of the system? f) Given the final temperature you have calculated for the system, what is the change in the length of the iron bar? (The coefficient of linear expansion of iron is 12x10–6 / ˚C ).

A block of metal of mass 0.200 kg is heated to 152.0°C and dropped in a copper calorimeter of mass 0.250 kg that contains 0.150 kg of water at 30°C. The calorimeter and its contents are insulated from the environment and have a final temperature of 46.0°C upon reaching thermal equilibrium. Find the specific heat of the metal. Assume the specific heat of water is 4.190 × 103 J/(kg · K) and the specific heat of copper is 386 J/(kg · K). J/(kg · K)

Ice at 0 °C is placed in a Styrofoam cup containing 0.62 kg of lemonade at 32 °C. The specific heat capacity of lemonade is virtually the same as that of water; that is, c = 4180 J/(kg C°). After the ice and lemonade reach an equilibrium temperature, some ice still remains. The latent heat of fusion for water is Lf = 3.35 x 105 J/ kg. Assume that the mass of the cup is so small that it absorbs a negligible amount of heat, and ignore any heat lost to the surroundings. Determine the mass of ice that has melted, in grams.

Consider a 10.0 kg iron box holding 48.0 kg of solid ice. Initially, both the box and the ice are at −35.0 ̊C. You put the box on an electric heater, which has a power output of 9580 Watts. Assume that all of the energy produced by the heater goes into heating the box and the ice. The specific heat of iron is 450.0 J kg−1 ̊C−1, the specific heat of ice is 2108 J kg−1 ̊C−1, and the latent heat of fusion of ice is 333500 J kg−1. (a)How much energy is required to heat the box and the ice to the melting point of ice (0 ̊C)? Give your answer in Joules. (b)How much energy (in Joules) is required to then melt all of the ice?