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Problem3 A block of copper has a mass of 100 kg and an initial temperature of...
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped...
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped into a large lake at 15°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and the lake water. Determine the total entropy change for this process. The specific heat of Iron at room temperature is cp0.45 kJ/kg.K. The specific heat of copper at 27°C is ep 0,386 kJ/kg.K. Iron Lake 15°C Copper The total entropy change...
Problem 2: (10 pts) A 30-kg iron block at initial temperature 200°C and a 40-kg copper...
Problem 2: (10 pts) A 30-kg iron block at initial temperature 200°C and a 40-kg copper block at initial temperature 100°C are dropped into a very large lake at 20°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and lake water. Both blocks have constant specific heats, i.e. Ciron = 0.45 kJ/kg. K and Ccopper = 0.386 kJ/kg. K. Hint: The very large lake can be treated as a heat reservoir and...
6: A 50 kg copper block initially at 80 C is dropped into a lake at...
6: A 50 kg copper block initially at 80 C is dropped into a lake at 15 C. Thermal equilibrium is established after a while as a resul the lake water. The specific heat copper at roorm temperature is c,-0.386 kJ/kg°C. Assuming the surroundings to be at 20 c t of heat transfer between the b lock and a. Determine the internal energy change and the entropy change of the copper. b. Determine the total entropy change for this process....
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains...
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is Cp= 4.18 kJ/kg-K. The density of water is 997 kg/m3. The specific heat of copper at 27°C is cp=0.386 kJ/kg-K. Water Copper 90 L The final equilibrium temperature is 15.85 K. The total entropy change during this...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90 L of water at 10'C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp=418 kJ/kg-K. The density of water is 997 kg/m2. The specific heat of copper at 27°C is Cp=0.386 kJ/kg.K. Water Copper 90 L The final equilibrium temperature is OK The total entropy change during this process is OKJ/K.
A 3.2 kg block of copper at a temperature of 82°C is dropped into a bucket...
A 3.2 kg block of copper at a temperature of 82°C is dropped into a bucket containing a mixture of ice and water whose total mass is 1.2 kg. When thermal equilibrium is reached the temperature of the water is 8°C. How much ice was in the bucket before the copper block was placed in it? (Neglect the heat capacity of the bucket.) answer in kg
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C...
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C is added to 1.0 kg liquid water at 80 °C in an insulated container at constant atmospheric pressure. The copper has a heat capacity of 0.01 kJ kg1 and the specific heat of water is 4.2 kJ kg1 K (both assumed constant with temperature) c) Calculate the change in entropy of the system in b). s it appropriate to...
After transfer of 1.50 kJ of thermal energy to a 0.675-kg block of copper the temperature...
After transfer of 1.50 kJ of thermal energy to a 0.675-kg block of copper the temperature is 49.1 °C. The specific heat capacity of copper is 0.385 Jg oc1 Calculate the initial temperature of the copper. oC
Two copper blocks, each of mass 1.25 kg, one at 54°C and the other at 0eC,...
Two copper blocks, each of mass 1.25 kg, one at 54°C and the other at 0eC, are placed in contact in an isolated container (so no heat can escape) and allowed to come to equilibrium. Calculate the final temperature of the two blocks (in K), the entropy change of each (in נ-K 1), and AStot (in נ-K 1). The specific heat capacity of copper is 0.3853-K 1-g 1 and may be assumed constant over the temperature range involved final temperature...
After transfer of 1.60 kJ of thermal energy to a 0.451-kg block of copper the temperature...
After transfer of 1.60 kJ of thermal energy to a 0.451-kg block of copper the temperature is 44.1 °C. The specific heat capacity of copper is 0.385 J g-1 °C-1. Calculate the initial temperature of the copper.
A 34 kg iron block and a 48-kg copper block, both initially at 80°C, are dropped into a large lake at 15°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and the lake water. Determine the total entropy change for this process. The specific heat of Iron at room temperature is cp0.45 kJ/kg.K. The specific heat of copper at 27°C is ep 0,386 kJ/kg.K. Iron Lake 15°C Copper The total entropy change...
Problem 2: (10 pts) A 30-kg iron block at initial temperature 200°C and a 40-kg copper block at initial temperature 100°C are dropped into a very large lake at 20°C. Thermal equilibrium is established after a while as a result of heat transfer between the blocks and lake water. Both blocks have constant specific heats, i.e. Ciron = 0.45 kJ/kg. K and Ccopper = 0.386 kJ/kg. K. Hint: The very large lake can be treated as a heat reservoir and...
6: A 50 kg copper block initially at 80 C is dropped into a lake at 15 C. Thermal equilibrium is established after a while as a resul the lake water. The specific heat copper at roorm temperature is c,-0.386 kJ/kg°C. Assuming the surroundings to be at 20 c t of heat transfer between the b lock and a. Determine the internal energy change and the entropy change of the copper. b. Determine the total entropy change for this process....
A 46 kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is Cp= 4.18 kJ/kg-K. The density of water is 997 kg/m3. The specific heat of copper at 27°C is cp=0.386 kJ/kg-K. Water Copper 90 L The final equilibrium temperature is 15.85 K. The total entropy change during this...
A 70-kg copper block initially at 140'C is dropped into an insulated tank that contains 90 L of water at 10'C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp=418 kJ/kg-K. The density of water is 997 kg/m2. The specific heat of copper at 27°C is Cp=0.386 kJ/kg.K. Water Copper 90 L The final equilibrium temperature is OK The total entropy change during this process is OKJ/K.
a) Define entropy as a thermodynamic state variable. b) Determine the final temperature when a block of copper at 0 °C is added to 1.0 kg liquid water at 80 °C in an insulated container at constant atmospheric pressure. The copper has a heat capacity of 0.01 kJ kg1 and the specific heat of water is 4.2 kJ kg1 K (both assumed constant with temperature) c) Calculate the change in entropy of the system in b). s it appropriate to...
After transfer of 1.50 kJ of thermal energy to a 0.675-kg block of copper the temperature is 49.1 °C. The specific heat capacity of copper is 0.385 Jg oc1 Calculate the initial temperature of the copper. oC
Two copper blocks, each of mass 1.25 kg, one at 54°C and the other at 0eC, are placed in contact in an isolated container (so no heat can escape) and allowed to come to equilibrium. Calculate the final temperature of the two blocks (in K), the entropy change of each (in נ-K 1), and AStot (in נ-K 1). The specific heat capacity of copper is 0.3853-K 1-g 1 and may be assumed constant over the temperature range involved final temperature...
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