10.0 g of aluminum at 2.00 × 102 °C and 20.0 g of copper are placed...
10.0 g of aluminum at 2.00 × 102 °C and 20.0 g of copper are placed into a well-insulated container with 50.0 cm3 of ethanol at 21.0 °C. The combined system reaches an equilibrium temperature of 25.0 °C. Assume the temperature changes in the container itself can be safely ignored. What was the initial temperature of the copper?
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10.0 g of aluminum at 2.00 × 102 °C and 20.0 g of copper are
placed...
A cube of copper with a mass of 2.00 kg, initially at a temperature of 150.0°C,...
A cube of copper with a mass of 2.00 kg, initially at a temperature of 150.0°C, is in a well-insulated container. Water at a temperature of 22.0°C is added to the container, and the entire interior of the container is allowed to come to thermal equilibrium, where it reaches a final temperature of 67.0°C. What mass of water (in kg) was added? Assume any water turned to steam subsequently recondenses. kg
- IUI ILALUUUR VIWCUSE) 1. A 145 g sample of copper metal at 100.0°C is placed...
- IUI ILALUUUR VIWCUSE) 1. A 145 g sample of copper metal at 100.0°C is placed into 250.0 g of water at 25.0°C in a calorimeter. When the system reaches thermal equilibrium, the temperature of the water in the calorimeter is 28.8°C. Assume the calorimeter is perfectly insulated. What is the specific heat capacity of copper?
A combination of 0.250 kg of water at 20.0°C, 0.400 kg of aluminum at 26.0°C, and...
A combination of 0.250 kg of water at 20.0°C, 0.400 kg of aluminum at 26.0°C, and 0.100 kg of copper at 100°C is mixed in an insulated container and allowed to come to thermal equilibrium. Ignore any energy transfer to or from the container. What is the final temperature of the mixture?
A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed...
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL H2O initially at 25.0°C and allowed to reach
thermal equilibrium. What is the final temperature of the copper
and water given that the specific heat of copper is 0.385J/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
A 21.0 g sample of aluminum, which has a specific heat capacity of 0.897 J g...
A 21.0 g sample of aluminum, which has a specific heat capacity of 0.897 J g '°C ', is dropped into an insulated container containing 200.0 g of water at 25.0 °C and a constant pressure of 1 atm. The initial temperature of the aluminum is 90.1 °C Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. x10 ? X
3. A 100 g block of copper initially at 60°C is placed in contact with a...
3. A 100 g block of copper initially at 60°C is placed in contact with a 300 g block of aluminum initially at 30°C in an insulated container. A. Identify the block that loses thermal energy. (5 pts) B. Calculate the final equilibrium temperature of the two blocks. (15 pts) Copper a(Cu) = 17 x 10-61°C Ccu = 0.0923 cal/g.K = 386 J/kg-K LF (Cu) = 207 kJ/kg
12.0 g of aluminum at 200∘C and 22.0 g of copper are dropped into 50.0 cm3...
12.0 g of aluminum at 200∘C and 22.0 g of copper are dropped into 50.0 cm3 of ethyl alcohol at 15.0∘C. The temperature quickly comes to 28.0 ∘C What was the initial temperature of the copper in ∘C?
Physics 10.0 g of aluminum at 200Cand 22.0 g of copper are dropped into 53.0 cm3...
Physics
10.0 g of aluminum at 200Cand 22.0 g of copper are dropped into 53.0 cm3 of ethyl alcohol at 15.0 °C. The temperature quickly comes to 26.0°C What was the initial temperature of the copper in°C? Express your answer with the appropriate units. - 26.3 SubmitPrev Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0...
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0 g of water (C = 4.18 J/gº) initially at 21.0 °C in an insulated container. The system comes to thermal equilibrium (the metal and the water are at the same temperature) at 23.1 ° C. Calculate the specific heat of the metal. C=/ 8°C)
Two 20.0-g ice cubes at -10.0 degree C are placed into 205 g of water at...
Two 20.0-g ice cubes at -10.0 degree C are placed into 205 g of water at 25.0 degree C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
- IUI ILALUUUR VIWCUSE) 1. A 145 g sample of copper metal at 100.0°C is placed into 250.0 g of water at 25.0°C in a calorimeter. When the system reaches thermal equilibrium, the temperature of the water in the calorimeter is 28.8°C. Assume the calorimeter is perfectly insulated. What is the specific heat capacity of copper?
A
hot lump of 32.3 g of copper at an initial temperature of 96.5°C is
placed in 50.0 mL H2O initially at 25.0°C and allowed to reach
thermal equilibrium. What is the final temperature of the copper
and water given that the specific heat of copper is 0.385J/g°C and
the specific heat of water is 4.184J/g°C?
4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
A 21.0 g sample of aluminum, which has a specific heat capacity of 0.897 J g '°C ', is dropped into an insulated container containing 200.0 g of water at 25.0 °C and a constant pressure of 1 atm. The initial temperature of the aluminum is 90.1 °C Assuming no heat is absorbed from or by the container, or the surroundings, calculate the equilibrium temperature of the water. Be sure your answer has 3 significant digits. x10 ? X
3. A 100 g block of copper initially at 60°C is placed in contact with a 300 g block of aluminum initially at 30°C in an insulated container. A. Identify the block that loses thermal energy. (5 pts) B. Calculate the final equilibrium temperature of the two blocks. (15 pts) Copper a(Cu) = 17 x 10-61°C Ccu = 0.0923 cal/g.K = 386 J/kg-K LF (Cu) = 207 kJ/kg
Physics
10.0 g of aluminum at 200Cand 22.0 g of copper are dropped into 53.0 cm3 of ethyl alcohol at 15.0 °C. The temperature quickly comes to 26.0°C What was the initial temperature of the copper in°C? Express your answer with the appropriate units. - 26.3 SubmitPrev Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
QUESTION 1 A 34.6 g piece of metal, initially at 96.0 °C is placed in 50.0 g of water (C = 4.18 J/gº) initially at 21.0 °C in an insulated container. The system comes to thermal equilibrium (the metal and the water are at the same temperature) at 23.1 ° C. Calculate the specific heat of the metal. C=/ 8°C)
Two 20.0-g ice cubes at -10.0 degree C are placed into 205 g of water at 25.0 degree C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
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