3. A 100 g block of copper initially at 60°C is placed in contact with a...
Calculate the total amount of heat required to completely convert 500 g of ice at 0°C to liquid water at 50°C. (5 pts) Aluminum (Al) - 23 x 10°C c, = 0.215 cal/g K = 900 J/kg.K L = 395 kJ/kg Copper a(Cu) - 17 x 10/°C c. = 0.0923 cal/g.K = 386 J/kg.K Lc-207 kJ/kg Silver a(Ag) = 18 x 10*/°C c, -0.0558 cal/g.K = 233 J/kg.K L = 105 kJ/kg Water c =1 cal/g.K = 4187 J/kg.K =...
A 30.5 g sample of copper at 99.8 °C is carefully placed into an insulated container containing 207 g of water at 18.5 °C. Calculate the final temperature when thermal equilibrium is reached. Assume there is no energy transferred to or from the container. Specific heat capacities: Cu =0.385 Jg-loc- H20 - 4.184 Jgloc!
A 750 g block of copper is heated to 250 degrees C. It is placed in a 350 g aluminum vessel that contains 200 g of water at 5.00 degrees C. What is the final temperature of the copper, water, and aluminum vessel? Specific heat of copper = 0.093 cal/g C degrees Specific heat of aluminum = 0.215 cal/g C degrees Specific heat for water = 1.0 cal/g C degrees
An aluminum block weighing 32 kg initially at 140°C is brought into contact with a block of iron weighing 44 kg at 60°C in an insulated enclosure. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of aluminum at 400 K is Cp0.949 kJ/kg.K. The specific heat of iron at room temperature is Cp=0.45 kJ/kg.K. The final equilibrium temperature is 108,35 K. The total entropy change for this process is 397 kJ/K
A 100 g block of copper (p = 8900 kg/m^3) and a 100 g block of aluminum (p = 2700 kg/m^3) are connected by a massless string that runs over two massless, frictionless pulleys. The two blocks exactly balance, since they have the same mass. Now suppose the two blocks are submerged in water. What will happen? The copper block will fall, the aluminum block will rise. The aluminum block will fall, the copper block will rise. Nothing will change...
A 4.31 kg block of Copper at +275oC is placed into thermal contact with a block of ice at +0.000oC. When they reach thermal equilibrium, the final temperature of everything is 0.000oC and only HALF of the ice has melted into water! What was the original amount of ice (in kg)?
Problem 7.30 You place into an insulated container a 1.8 kg block of aluminum at a temperature of 43°C in contact with a 2.4 kg block of copper at a temperature of 18°C. The specific heat of aluminum is 0.91 J/K/g and the specific heat of copper is 0.391/K/g, what is the final temperature of the two blocks? oC the tolerance is +/-296
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...
A 4.1-kg block of ice originally at 263 K is placed in thermal contact with a 13.1-kg block of silver (cAg = 233 J/kg-K) which is initially at 1064 K. The H2O - silver system is insulated so no heat flows into or out of it. 1) At what temperature will the system achieve equilibrium? ________K
A 4.2-kg block of ice originally at 263 K is placed in thermal contact with a 13.7-kg block of silver (cAg = 233 J/kg-K) which is initially at 1086 K. The H2O - silver system is insulated so no heat flows into or out of it. 1)At what temperature will the system achieve equilibrium? K