An 5.0 g ice cube at -24.0?C is put into a Thermos flask containing 125 cm3...

An 5.0 g ice cube at -24.0?C is put into a Thermos flask containing 125 cm3 of water at 20.0?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

Expert Solution

initially the ice warms from -24 oC to 0 oC
The change in entropy in this case is
       ?S1 = integral ( dQ /T)
              = m C_ice ln (Tf / Ti)
              = (5 x 10^-3) (2200) ln (273 / 259)
              = 0.579 J/ K
Now the ice melts at 0^oC , Then
       ?S2 = Q / T = mL /T   = 5 * 333 / 273 = 6.09J /K
Now the water warms to lake temperature
         ?S3 = m Cw ln(Tf / Ti)
                = (5 / 1000) (4187) ln (293 / 273)
                = 1.48 J /K
Therefore total change in entropy
         ?S = 0.579 +6.09 + 1.48= 8.149 J /K

genius_generous answered 1 hour ago

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.

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.)

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 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?

An insulated Thermos contains 123 g of water at 83.0 ˚C. You put in a 7.92...

An insulated Thermos contains 123 g of water at 83.0 ˚C. You put in a 7.92 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 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

Question