A hot block of iron is placed on top of a block of ice at Ti...
A hot block of iron is placed on top of a block of ice at Ti water = -60° C in an insulating container so no heat can be transferred into or out of the container. When you open the container later the ice has completely melted. For the physical system of the iron and water, what energy systems changed from the time the iron is placed insided to the time the container is opened
Homework Answers
Since System of ice and hot iron is in insulated container so there is no energy and mass exchange between system and its surrounding.
Its mass and energy content will remain same so Change in energy of sysyem will be zero.
Energy given by hot iron is equal to energy taken by ice.
A hot block of iron is placed on top of a block of ice at Tiwater--60°...
A hot block of iron is placed on top of a block of ice at Tiwater--60° C in an insulating container so no heat can be transferred into or out of the container. When you open the container later the ice has completely melted. For the physical system of the iron and water, what energy systems changed from the time the iron is placed insided to the time the container is opened? Ebond, water O Ethermal, iron, Ethermal, water Ethermal...
1) A block of iron at Tiiron- 500°C is placed on top of a block of...
1) A block of iron at Tiiron- 500°C is placed on top of a block of ice (solid water) at Ti water-50°C in an insulating container so no heat can be transferred into or out of the container. Parts of the graphs of Tvs energy added for the three-phase model are shown to the right. Use these graphs to find the approximate final equilibrium temperatures, Tf iron and Tfwater, the final phases of the iron and water, and the approximate...
A block of ice, mass 3.21 kg and initial temperature of -15 oC, is placed in...
A block of ice, mass 3.21 kg and initial temperature of -15 oC, is placed in an insulating container. 3.22 kg of water at temperature 25 oC, is added to the container. The water and ice exchange heat, but no other heat flows into or out of the container. In the process of the water and ice reaching equilibrium, how much ice melts? Give your answer in kg to three digits.
A block of ice, mass 2.16 kg and initial temperature of -8 oC, is placed in...
A block of ice, mass 2.16 kg and initial temperature of -8 oC, is placed in an insulating container. 3.12 kg of water at temperature 24 oC, is added to the container. The water and ice exchange heat, but no other heat flows into or out of the container. In the process of the water and ice reaching equilibrium, how much ice melts? Give your answer in kg to three digits. Note: It is possible that the answer is zero.
You make a cup of hot coffee and pour it into an insulated container that already...
You make a cup of hot coffee and pour it into an insulated container that already has ice in it. Assume that the insulated container itself has a very small heat capacity so that any energy transferred from it or to it is negligible and can be ignored. What energy systems are changing. starting from when you pour the coffee into the insulated container to when the ice is completely melted and the mixture has a uniform temperature? Ethermal, coffee,...
a hot piece of iron at 75 degrees celsius was dropped on a 15g ice cube...
a hot piece of iron at 75 degrees celsius was dropped on a 15g ice cube at 0 degrees celsius. after a few minutes, both the iron and the water stayed at 0 degrees celsius but the ice melted completely. what is the mass of the iron? (Ciron = 0.0449 J/g degrees celsius, △Hfus = 6.00 kJ/mol)
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is...
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is 30 percentage ice and the rest water that is in an iron container that has a mass of 2kg. Assume the ice bath and iron container is at thermal equilibrium to start. The final equilibrium temperature is 37 degree C. How much energy input is needed to convert the ice to water? Assuming no energy is lost to the environment and the system is...
An 810-g iron block is heated to 400 ∘C and placed in an insulated container (of...
An 810-g iron block is heated to 400 ∘C and placed in an insulated container (of negligible heat capacity) containing 38.0 g of water at 25.0 ∘C. What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg⋅K).
An 900-g iron block is heated to 380 ∘C and placed in an insulated container (of...
An 900-g iron block is heated to 380 ∘C and placed in an insulated container (of negligible heat capacity) containing 36.0 g of water at 20.0 ∘C. What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg⋅K).
An 870-g iron block is heated to 370 C and placed in an insulated container (of...
An 870-g iron block is heated to 370 C and placed in an insulated container (of negligible heat capacity) containing 41.0g of water at 21.0 C. What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kgxK). What is the equilibrium temperature of this system? The average specific heat of iron over this temperature range is 560 J/(kg?K).
A hot block of iron is placed on top of a block of ice at Tiwater--60° C in an insulating container so no heat can be transferred into or out of the container. When you open the container later the ice has completely melted. For the physical system of the iron and water, what energy systems changed from the time the iron is placed insided to the time the container is opened? Ebond, water O Ethermal, iron, Ethermal, water Ethermal...
1) A block of iron at Tiiron- 500°C is placed on top of a block of ice (solid water) at Ti water-50°C in an insulating container so no heat can be transferred into or out of the container. Parts of the graphs of Tvs energy added for the three-phase model are shown to the right. Use these graphs to find the approximate final equilibrium temperatures, Tf iron and Tfwater, the final phases of the iron and water, and the approximate...
You make a cup of hot coffee and pour it into an insulated container that already has ice in it. Assume that the insulated container itself has a very small heat capacity so that any energy transferred from it or to it is negligible and can be ignored. What energy systems are changing. starting from when you pour the coffee into the insulated container to when the ice is completely melted and the mixture has a uniform temperature? Ethermal, coffee,...
A hot gold bar that is 45kg is lowered into a 20kg ice bath that is 30 percentage ice and the rest water that is in an iron container that has a mass of 2kg. Assume the ice bath and iron container is at thermal equilibrium to start. The final equilibrium temperature is 37 degree C. How much energy input is needed to convert the ice to water? Assuming no energy is lost to the environment and the system is...
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