An 13 g ice cube at -13˚C is put into a Thermos flask containing 110 cm3...

An 13 g ice cube at -13˚C is put into a Thermos flask containing 110 cm3 of water at 18˚C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg.

Expert Solution

genius_generous answered 2 years ago

An 7.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3...

An 7.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3 of water at 21°C. By how much has the entropy of the cube–water system changed when equilibrium is reached? The specific heat of ice is 2220 J/kg · K. (The latent heat of fusion for water is 333 kJ/kg.)

An 8.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3...

An 8.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3 of water at 30°C. By how much has the entropy of the cube-water system changed when equilibrium is reached? The specific heat of ice is 2220 J/kg · K. (The latent heat of fusion for ice is 333 kJ/kg and the specific heat of water is 4187 J/kg · K.)

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0...

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5...

An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

A 1.10 −g sample of dry ice is added to a 765 −mL flask containing nitrogen...

A 1.10 −g sample of dry ice is added to a 765 −mL flask containing nitrogen gas at a temperature of 25.0 ∘C and a pressure of 715 mmHg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 ∘C. What is the total pressure in the flask? Express your answer using three significant figures.

An ice cube of mass 0.029 kg and temperature -13 ∘C is dropped into a styrofoam...

An ice cube of mass 0.029 kg and temperature -13 ∘C is dropped into a styrofoam cup containing water of mass 0.4 kg and temperature 20 ∘C. Calculate the final temperature in degrees celcius and give your answer to one decimal place. (For simplicity, we ignore here the temperature change of the cup.) The specific heat of ice is 2200 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is...

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in...

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in an 80-g aluminum container, both initially at 30°C. What is the final equilibrium temperature? (Specific heat for aluminum is 900 J/kg×°C, the specific heat of water is 4 186 J/kg×°C, and Lf = 3.33 ´ 105 J/kg.)

a) A(n) 85-g ice cube at 0°C is placed in 920 g of water at 20°C....

a) A(n) 85-g ice cube at 0°C is placed in 920 g of water at 20°C. What is the final temperature of the mixture? b) A 103-g cube of ice at 0°C is dropped into 1.0 kg of water that was originally at 87°C. What is the final temperature of the water after the ice has melted? c) An aluminum cup contains 225 g of water and a 40-g copper stirrer, all at 27°C. A 432-g sample of silver at...

The density of ice is 920 kg/m3. If an ice cube is put in a beaker...

The density of ice is 920 kg/m3. If an ice cube is put in a beaker of water collected from the Great Salt Lake it floats with 80% of its volume submerged. What is the density of the water collected from the Great Salt Lake? 736 kg/m3 1000 kg/m3 1080 kg/m3 1150 kg/m3 none of the above

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that...

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that was originally 84.1∘C. What is the final temperature of the water after the ice melts and the water comes to thermal equilibrium? This problem requires a lot of algebra. You will make fewer errors if you solve for the answer using symbols and then plug in the numbers. The specific heat of water and the latent heat of fusion for water are given in...

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