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
heat gained by ice = Mice*Cice*dT1 + mice*Lf +
mice*cw*dT2
Qgain = (4.1*2100*(273-263)) +
(4.1*334000)+(4.1*4190*(T-273))
Qgain = 1455500 + 17179T - 4689867
Qgain = 17179T - 3.234367e+6
heat lost by silver = mAg*cAg*dT3
Qloss = 13.2*233*(1064-T) = 3272438.4 -
3075.6T
from pricilple of calorimetry
Qlosss = Q gain
3272438.4 - 3075.6T = 17179T - 3.234367e+6
T = 321 K
A 4.1-kg block of ice originally at 263 K is placed in thermal contact with a...
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
A 4.4-kg block of ice originally at 263 K is placed in thermal contact with a 14.4-kg block of silver (CAg - 233 J/kg-K) which is initially at 1007 K. The H2O-silver system is insulated so no heat flows into or out of it. (Note: Cice- 2050 J/kg-K) 1) At what tepeature will the system achieve equilibrium? KI Submit A 4.4-kg block of ice originally at 263 K is placed in thermal contact with a 14.4-kg block of silver (CAg...
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)?
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
The following three substances are placed together in thermal contact: 1) Mg = 1.0 kg gold at temperature Tg = −13 C 2) Ms = 2.0 kg silver at temperature Ts = +7.0 C 3) Mi = 0.01 kg ice at temperature Ti = 0.0 C What is the final equilibrium temperature T ? Data: specific heat of ice: Ci = 2100 specific latent heat of fusion of ice/water: Lf = 3.35 × 10^5 specific heat of gold: Cg =...
A 0.0575 kg ice cube at −30.0°C is placed in 0.617 kg of 35.0°C water in a very well insulated container, like the kind we used in class. The heat of fusion of water is 3.33 x 105 J/kg, the specific heat of ice is 2090 J/(kg · K), and the specific heat of water is 4190 J/(kg · K). The system comes to equilibrium after all of the ice has melted. What is the final temperature of the system?
A 0.0725 kg ice cube at −30.0°C is placed in 0.497 kg of 35.0°C water in a very well insulated container, like the kind we used in class. The heat of fusion of water is 3.33 x 105 J/kg, the specific heat of ice is 2090 J/(kg · K), and the specific heat of water is 4190 J/(kg · K). The system comes to equilibrium after all of the ice has melted. What is the final temperature of the system?
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
(15 points) An ice cube of mass 0.0340 kg and temperature -10.00 °C is placed in the steam room at a gym. The steam room, which is quite large, is filled with 2.000 kg of steam at a temperature of 110.0 °C (a) (5 points) How much ice is present, and at what temperature, when the ice and steam reach thermal equilibrium? Your answer should be two numbers (b) (5 points) How much water is present, and at what temperature,...
An aluminium block is heated to 100 °C and then placed immediately in 100 g of water which is initially at a temperature of 25.0 °C in a coffee cup calorimeter. Once the system reaches thermal equilibrium, the temperature of the water that surrounds the block is 28.0 °C. Calculate the mass of the aluminium block. The specific heat capacity of Al is 0.900 J g^–1 K^–1 and for H2O is 4.184 J g^–1 K^–1