A lab assistant pours 330 g of water at 45°C into an 855-g aluminum container that is at an initial temperature of 10°C. The specific heat of aluminum is 900 J/kg ∙ K and that of water is 4186 J/kg ∙ K. What is the final temperature of the system, assuming no heat is exchanged with the surroundings?

A 53.5 g silver block initially at 8.0°C is submerged in water initially at 83.5°C in an insulated container. The final temperature of both substances at thermal equilibrium is 78.5°C. What is the mass of the water? (The heat capacity of silver is 0.235 J/g°C, and the heat capacity of water is 4.18 J/g°C)

Suppose you place 0.265 kg of 24.5°C water in a 0.45 kg aluminum pan with a temperature of 147.5°C, and 0.0125 kg of the water evaporates immediately, leaving the remainder to come to a common temperature with the pan. What would be the final temperature, in degrees Celsius, of the pan and water? The heat of vaporization of water is Lv = 2256 kJ/kg. You may neglect the effects of the surroundings and the heat required to raise the temperature of the vaporized water.  Te =

Large steel plates 1.0-cm in thickness are quenched from 600°C to 100°C by submerging them in an oil reservoir held at 30°C. The average heat transfer coefficient for both faces of steel plates is 400 W/m2·K. Average steel properties are k = 45 W/m·K, r = 7800 kg/m3, and cp = 470 J/kg·K. Calculate the quench time for steel plates.

A 0.70-kg piece of metal is heated to 80.0 °C and dropped into an ideal calorimeter containing 1.2 kg of water initially at 30.0 °C. What is the final equilibrium temperature of the piece of metal? The specific heat capacity of the piece of metal is 140 J/(kg · C°); and the specific heat of water is 4186 J/(kg ·C°). Hint: start with Qin = Qout O a) 31.0 °C O b) 18.2 °C c) 21.5 O d) 24.5 °C e) 21.3 °C f) 32.6 °C

A 99.8-g aluminum calorimeter contains 258 g of water. The aluminum and water are initially in thermal equilibrium at a temperature of 9.5°C. Two solid objects are then placed in the water. One is a 48.3-g piece of copper with a specific heat of 390 J/(kg⋅°C) and an initial temperature of 80.5°C. The other is of unknown material with a mass of 68 g and an initial temperature of 100°C. The entire system reaches thermal equilibrium at a temperature of 20.2°C. The specific heats of aluminum and water are 910 J/(kg⋅°C) and 4186 J/(kg⋅°C), respectively.  -Find the specific heat of the unknown material, in units of J/(kg⋅°C).

Two blocks of metal are in contact with one another. The first block has mass 4.4 kg and specific heat 160 J/kg*K. The second block has mass 3.8 kg, specific heat 538 J/kg*K and temeperature 282 K. The final temperature of the system is 154 K. What was the initial temperature of the first block?

An unknown substance has a mass of 0.125 kg and an initial temperature of 94.5°C. The substance is then dropped into a calorimeter made of aluminum containing 0.285 kg of water initially at 25.5°C. The mass of the aluminum container is 0.150 kg, and the temperature of the calorimeter increases to a final equilibrium.temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance. J/kg - °C Need Help? Read It MY NOTES ASK YOUR TEACHER PRACTICE ANOTHER SERCP11 11.4.P.033.MI.

A 0.0725 kg ice cube at −30.0°C is placed in 0.557 kg of 35.0°C water in a very well insulated container. What is the final temperature? The latent heat of fusion of water is 79.8 kcal/kg, the specific heat of ice is 0.50 kcal/(kg · °C), and the specific heat of water is 1.00 kcal/(kg · °C).

A 283 g silver figure of a polar bear is dropped into the 249 g aluminum cup of a well-insulated calorimeter containing 265 g of liquid water at 20.9°C. The bear's initial temperature is 98.5°C. What is the final temperature of the water, cup, and bear when they reach thermal equilibrium? The specific heats of silver, aluminum, and liquid water are, respectively, 234 J/ (kg-K), 910 J/ (kg-K), and 4190 J/ (kg-K). final temperature: °C