The value of specific heat for copper is 390 J/kg⋅C∘J/kg⋅C∘, for aluminun is 900 J/kg⋅C∘J/kg⋅C∘, and for water is 4186 J/kg⋅C∘J/kg⋅C∘. What will be the equilibrium temperature when a 265 gg block of copper at 255 ∘C∘C is placed in a 155 gg aluminum calorimeter cup containing 815 gg of water at 15.0 ∘C∘C?

The value of specific heat for copper is 390 J/kg⋅C∘J/kg⋅C∘, for aluminun is 900 J/kg⋅C∘J/kg⋅C∘, and for water is 4186 J/kg⋅C∘J/kg⋅C∘. What will be the equilibrium temperature when a 265 gg block of copper at 255 ∘C∘C is placed in a 155 gg aluminum calorimeter cup containing 815 gg of water at 15.0 ∘C∘C?

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The value of specific heat for copper is 390 J/kg⋅∘C, for aluminum is 900 J/kg⋅∘C, and for water is 4186 J/kg⋅∘C. What will be the equilibrium temperature when a 265 g block of copper at 255 ∘C is placed in a 155 g aluminum calorimeter cup containing 815 g of water at 15.0 ∘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
A mFe = 0.16 kg mass of iron is heated to 100∘C and then placed in a Styrofoam cup containing mw = 0.50 kg of water. Initially, the water and has a temperature of 27∘C. Find the equilibrium temperature of the system. cw = 4186 J/kg∘C and cFe = 460 J/kg∘C.
The value of specific heat for copper is 390 J/kg⋅C∘J/kg⋅C∘, for aluminun is 900 J/kg⋅C∘J/kg⋅C∘, and for water is 4186 J/kg⋅C∘J/kg⋅C∘ What will be the equilibrium temperature when a 265 gg block of copper at 255 ∘C∘C is placed in a 155 gg aluminum calorimeter cup containing 815 gg of water at 13.0 ∘C∘C?
A 50.0-g piece of brass (specific heat 380 J/kg K) is heated to 90.0° C and immersed in 100 g of water (specific heat 4184 J/kg K), initially at 15.0° C c. The well-insulated container is then sealed and allowed to reach thermal equilibrium. What is the final temperature of the system? 18.3° C 13.7° С 24.8° C 36.3° C 12.9° C
A 390-g metal container, insulated on the outside, holds 170.0 g of water in thermal equilibrium at 21.0°C. A 18.0-g ice cube, at -15.0°C, is dropped into the water, and when thermal equilibrium is reached the temperature is 12.0°C. Assume there is no heat exchange with the surroundings. The specific heat capacity of water is 4190 J/kg ∙ K, the specific heat capacity of ice is 2090 J/kg ∙ K and the heat of fusion is 3.34 × 105 J/kg. What is the specific heat capacity of the metal of the container?
A cube of ice is taken from the freezer at -8.8°C and placed in a 104 g iron cup filled with 279 g of water. Both the water & the cup are at 23.9°C. Eventually the system reaches thermal equilibrium at 12.4°C. Determine Qcup, Qwater (for the water initially in the cup), Qice, & the mass of the ice.Qcup = Qwater = Qice = mice =
A well-insulated aluminum calorimeter cup with mass of 231 g contains 271 g of liquid water at 25.1 °C. A 295-g silver figure of polar bear, with initial temperature of 96.5 °C, is dropped into the water. 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:
A heavy pot made of copper has a mass of 2.24 kg (including the lid) and is heated in an oven to a temperature of 154 °C. You pour 0.12 kg of water at 26.0 °C into the pot and quickly close the lid so that no steam can escape. We assume that no heat is lost to the surrounding. For copper, Ccopper 390 J/(kg.K) For water, Cwater 4190 J/(kg.K), L, = 2256 kJ/kg, L; = 333 kJ/kg. %3D What is the final mass of steam in the pot? on
A silver block, initially at 56.9 ∘C∘C, is submerged into 100.0 gg of water at 24.1 ∘C∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.4 ∘C∘C. What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units.
A 0.100 kg piece of ice at initial temperature −5.00 ◦C is placed in a perfectly insulated container with 1.00 kg (1 L) of water at initial temperature 20.0 ◦C. The container absorbs or releases no heat. All of the ice melts as the system reaches an equilibrium temperature Tf . How much heat must the ice exchange with the rest of the system to raise its temperature to the melting point, 0.00 ◦C? Would this heat exchanged be positive, zero, or negative? Once the ice reaches its melting point, how much heat must the ice exchange with the rest of the system to melt? Would this heat exchanged be positive, zero, or negative? Once the ice melts, it is liquid water at 0.00 ◦C. Write an expression for the heat exchanged by the newly-melted ice QI to reach the equilibrium temperature Tf . Would you expect QI to be positive, zero, or negative? Write an expression for the heat exchanged by the original water QW to reach the equilibrium temperature Tf from its initial temperature. Assuming no…