Latent Heats: A beaker of negligible heat capacity contains 456 g of ice at -25.0°C. A lab technician begins to supply heat to the container at the rate of 1000 J/min. How long after starting will the ice begin to melt, assuming all of the ice has the same temperature? The specific heat of ice is 2090 J/kg ∙ K and the latent heat of fusion of water is 33.5 × 104 J/kg.

A 0.200-kg mass of metal with a specific heat of 1255.8 J/kg-°C, initially at 90°C, is placed in a 0.500-kg calorimeter, with a specific heat of 418.6 J/kg-°C, initially at 20°C. The calorimeter is filled with 0.100 kg of water, initially at 20°C. The specific heat of water is 4186 J/kg-°C. What is the final temperature once the combination of metal, calorimeter, and water reach equilibrium? O 70°C 40°C 60°C O 50°C

How much thermal energy (in J) is required to boil 2.45 kg of water at 100.0°C into steam at 135.0°C? The latent heat of vaporization of water is 2.26 ✕ 106 J/kg and the specific heat of steam is  2010  J kg · °C . HINT  J

In an electrically heated home, the temperature of the ground in contact with a concrete basement wall is 14.0 °C. The temperature at the inside surface of the wall is 21.4 °C. The wall is 0.12 m thick and has an area of 7.7 m2. Assume that one kilowatt hour of electrical energy costs $0.10. How many hours are required for one dollar's worth of energy to be conducted through the wall? Number Units the tolerance is +/-2%

In an insulated container, you combine hot metal with ice. The ice starts at -20 degree C. The copper starts at 900 degree C. When 15 kg of the copper is combined with an unknown amount of ice, the system reaches equilibrium as soon as all of the ice has boiled to become steam. What is the final temperature of the copper?

You drop an ice cube into an insulated container full of water and wait for the ice cube to completely melt. The ice cube initially has a mass of 60.0 g and a temperature of 0°C. The water (before the ice cube is added) has a mass of 850 g and an initial temperature of 30.0°C. What is the final temperature (in °C) of the mixture? (Assume no energy is lost to the walls of the container, or to the environment.)

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

In a physics lab, students are conducting an experiment to learn about the heat capacity of different materials. The first group is instructed to add a number of 1.50 g pellets made of lead, at a temperature of 92.0°C, to 305 g of water at 16.0°C. A second group is given the same number of 1.50 g pellets as the first group, but these are now aluminum pellets. Assume that no heat is lost to or gained from the surroundings for either group. (a) If the final equilibrium temperature of the lead pellets and water is 25.0°C, how many whole pellets did the first group use in the experiment? The specific heat of lead is 0.0305 kcal/(kg · °C). pellets (b) Will the final equilibrium temperature for the second group be higher, lower, or the same as for the first group? The specific heat of aluminum is 0.215 kcal/(kg · °C). O higher O lower O the same (c) What is the equilibrium temperature of the aluminum and water mixture for the second group? °C

You drop an ice cube into an insulated flask full of water and wait for the ice cube to completely melt. The ice cube initially has a mass of 90.0 g and a temperature of 0°C. The water (before the ice cube is added) has a mass of 850 g and an initial temperature of 22.0°C. What is the final temperature (in °C) of the mixture? (Assume no energy is lost to the walls of the flask, or to the environment.)  °C

A 1.50 kg block of ice initially at a temperature of 0 °C is placed inside an apparatus that allows 150 kJ of heat to flow into the ice. What mass of ice melts as a result? O 0.45 kg O 0.75 kg O 1.33 kg O 2.23 kg O 1.00 kg