How much heat energy is required to raise the temperature of 0.368 kgkg of copper from 23.0 ∘C∘C to 60.0 ∘C∘C? The specific heat of copper is 0.0920 cal/(g⋅∘C)cal/(g⋅∘C)

An insulated beaker with negligible mass contains liquid water with a mass of 0.210 kgkg and a temperature of 74.1 ∘C . How much ice at a temperature of -22.6 ∘C must be dropped into the water so that the final temperature of the system will be 32.0 ∘C? Take the specific heat of liquid water to be 4190 J/kg⋅KJ/kg⋅K , the specific heat of ice to be 2100 J/kg⋅KJ/kg⋅K , and the heat of fusion for water to be 3.34×105 J/kgJ/kg .

The specific heat of most solids is nearly constant over a wide temperature range. Not so for diamond. Between 200 K and 600 K, the specific heat of diamond is reasonably well described by c=2.8T−350J/kg⋅K, where T is in K. For gemstone diamonds, 1 carat = 200 mg. How much heat energy is needed to raise the temperature of a 2.5 carat diamond from -50∘C to 250 ∘C?

Suppose that on a dry, sunny day when the air temperature is near 37∘C, a certain swimming pool would increase in temperature by 1.75∘C in one hour if not for evaporation. What fraction of the water in the pool must evaporate during this time to carry away precisely enough energy to keep the temperature of the pool constant? The specific heat of water is 4186 J/(kg·∘C). At 37∘C, the latent heat of vaporization of water is 2430 kJ/kg. Assume that the water in the pool is close enough to 37 ∘C that this value for the latent heat can be used.

A styrofoam container used as a picnic cooler contains a block of ice at 0°C. If 564 g of ice melts in 1 hour, how much heat energy per second is passing through the walls of the container? The heat of fusion of ice is 3.33 x 10° J/kg. Answer in units of W.

A 2.80-kg steel ball at 24.7°C is dropped from a height of 15.4 m into an insulated container with 4.50 L of water at 10.1°C. If no water splashes, what is the final temperature of the water and steel? The specific heat of steel and water is 450 J/(kg·K) and 4186 J/(kg·K) respectively.

A closed box is filled with dry ice at a temperature of -88.3 oC, while the outside temperature is 18.8 oC. The box is cubical, measuring 0.309 m on a side, and the thickness of the walls is 3.80 × 10-2 m. In one day, 3.62 × 106 J of heat is conducted through the six walls. Find the thermal conductivity of the material from which the box is made.

Calculate the heat in kJ for 9.98 g of ice at -75.0 oC heated to -38.0 oC with a specific heat capacity of 2.087 J/(g·oC).

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).

1.2-kg of ice at -6.0°C is dropped into 5.0 L (5.566-kg) of car coolant. The initial temperature of the coolant is 25.0°C. The ice and coolant are insulated, so energy transfers to the outside is negligible. After hours, all ice melts and the final temperature of the mixture of water-coolant is 1.8°C. The specific heat of ice is 2090 J/kg °C; the specific heat of water is 4186 J/kg °C; the latent heat of fusion for water is 334000 J/kg. A. What is the energy needed for heating the ice to 0 °C? B. Determine the energy needed to melt the ice into water. C. Determine the total energy needed to heat the -6.0°C ice to 1.8°C water. (Please note: the total energy also includes the part heating water from 0.0 °C to 1.8 °C.) D. Determine the specific heat capacity of the coolant.