Suppose 125 g of ice at 0°C is added to 550 g of water at 85°C....
Suppose 125 g of ice at 0°C is added to 550 g of water at 85°C. What is the total change in entropy of the universe after it reaches thermal equilibrium? Show your work
Homework Answers
A 32.4-g ice cube at 0 °C is added to 125 g of water in a...
A 32.4-g ice cube at 0 °C is added to 125 g of water in a 63.3-g aluminum cup. The cup and the water have an initial temperature of 23.0 °C. Calculate the equilibrium temperature of the cup and its contents.Calculate the equilibrium temperature of the cup and its contents if the aluminum cup is replaced with one of equal mass made from silver. Please include work so I can understand. Thank you!
1.) 40 g of liquid water at 30 C and 20 g of ice at 0...
1.) 40 g of liquid water at 30 C and 20 g of ice at 0 C are mixed together in an insulated container. Assuming there is not heat lost to surroundings, what will the temperature be when the mixture has reached thermal equilibrium. (show your work) 2.)20 g of ice at 0 C and 10 g of steam at 100 C are mixed together in an insulated container. Assuming there is not heat lost to surroundings, what will the...
4. You drop 500 g of solid ice at 0°C into a 2 kg bucket of...
4. You drop 500 g of solid ice at 0°C into a 2 kg bucket of water at 40°C. Eventually everything comes to thermal equilibrium. A) What is the final temperature of the system? B) How much heat flowed into the ice? ) What was the entropy change of the ice that turned into water?
An ice cube of mass 500 g at 0 °C is dropped into an insulated container...
An ice cube of mass 500 g at 0 °C is dropped into an insulated container of 1.0 kg of water that initially is at room temperature (25 °C), and eventually the system reaches equilibrium. The insulator is not perfect, so 20 kJ of heat flows from the room into the water during the process. 3. a. Calculate the entropy increase in the ice that melts into water. b. Calculate the entropy loss of the water that cools down. c....
4. If 161 g of water at 85°C is cooled to ice at 0°C, find the...
4. If 161 g of water at 85°C is cooled to ice at 0°C, find the change in heat content of the system.
A. A 32.1 g of ice at 0 C is added to 120g of water in...
A. A 32.1 g of ice at 0 C is added to 120g of water in a 64.8 g aluminum cup. the cup and the water have an initial temperature of 23.7 C. Calculate the equilibrium temperature of the cup and its contents. B. Calculate the equilibrium temperature of the cup and its contents if the aluminum cup is replaced with one of equal mass made from glass.
A 33.3-g ice cube at 0 °C is added to 126 g of water in a...
A 33.3-g ice cube at 0 °C is added to 126 g of water in a 62.5-g aluminum cup. The cup and the water have an initial temperature of 24.3 °C. Calculate the equilibrium temperature of the cup and its contents. Do not enter unit. Calculate the equilibrium temperature of the cup and its contents if the aluminum cup is replaced with one of equal mass made from copper. Do not enter unit.
A quantity of ice at 0 degree C is added to 50 g of water in a glass at 55 degree C. After the ice melted, the temperatu...
A quantity of ice at 0 degree C is added to 50 g of water in a glass at 55 degree C. After the ice melted, the temperature of the water was 15 degree C. How much ice was added?
Three 101.0-g ice cubes initially at 0°C are added to 0.820 kg of water initially at...
Three 101.0-g ice cubes initially at 0°C are added to 0.820 kg of water initially at 19.5°C in an insulated container. (a) What is the equilibrium temperature of the system? °C (b) What is the mass of unmelted ice, if any, when the system is at equilibrium? kg
Three 110.0-g ice cubes initially at 0°C are added to 0.900 kg of water initially at...
Three 110.0-g ice cubes initially at 0°C are added to 0.900 kg of water initially at 21.0°C in an insulated container. (a) What is the equilibrium temperature of the system? 9.13 Your response differs significantly from the correct answer. Rework your solution from the beginning and check each step carefully.°C (b) What is the mass of unmelted ice, if any, when the system is at equilibrium? The correct answer is not zero. kg
4. You drop 500 g of solid ice at 0°C into a 2 kg bucket of water at 40°C. Eventually everything comes to thermal equilibrium. A) What is the final temperature of the system? B) How much heat flowed into the ice? ) What was the entropy change of the ice that turned into water?
An ice cube of mass 500 g at 0 °C is dropped into an insulated container of 1.0 kg of water that initially is at room temperature (25 °C), and eventually the system reaches equilibrium. The insulator is not perfect, so 20 kJ of heat flows from the room into the water during the process. 3. a. Calculate the entropy increase in the ice that melts into water. b. Calculate the entropy loss of the water that cools down. c....
4. If 161 g of water at 85°C is cooled to ice at 0°C, find the change in heat content of the system.
Three 110.0-g ice cubes initially at 0°C are added to 0.900 kg of water initially at 21.0°C in an insulated container. (a) What is the equilibrium temperature of the system? 9.13 Your response differs significantly from the correct answer. Rework your solution from the beginning and check each step carefully.°C (b) What is the mass of unmelted ice, if any, when the system is at equilibrium? The correct answer is not zero. kg
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