After transfer of 1.50 kJ of thermal energy to a 0.675-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.
lerences TUTOR Combined Gas Law A 6.95 L sample of gas has a pressure of 1.5 atm and a temperature of 95°C. The sample is compressed to a volume of 5.75 L and is cooled to 39 C. Calculate the new pressure of the gas, assuming that no gas escaped during the experiment Submit Show Approach Show to Steps After transfer of 1.50 kJ of thermal energy to a 0.496-kg block of copper the temperature is 47.5 °C. The specific...
Problem3 A block of copper has a mass of 100 kg and an initial temperature of 900 K. Copper can be modeled as an incompressible substance with a specific heat capacity of 0.4 kJ/kg-K. a) The copper block is dropped into a large lake at 300 K and allowed to come to thermal equilibrium. How much entropy is generated (kJ/K)?
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...
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...
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 sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.
The change in entropy of a 1.50 kg block of copper whose temperature is increased reversibly from 310 K to 390 K is: (The specific heat of copper is 386 J/kg K)
Seperate the Fe and Cu answers by commas. PhET Simulation - Energy Forms and Changes 3 of 11 > A 1.2 kg block of iron at 36 c is rapidly heated by a torch such that 15 kJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (15 kJ ) was quickly transferred to a 810 pellet of copper...
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...