s = Q/T ... by definition of entropy
Q = mc dT = 0.039 x 2220 x (65-(-69))
= 11601.7 J
T= 65+273 = 338K
s = 34.32 J/K
A 39 g ice cube at -69°C is placed in a lake whose temperature is 65°C....
A 24 g ice cube at -26°C is placed in a lake whose temperature is 26°C. Calculate the change in entropy of the cube-lake system as the ice cube comes to thermal equilibrium with the lake. The specific heat of ice is 2220 J/kg·K. (Hint: Will the ice cube affect the temperature of the lake?)
A 82 g ice cube at -90°C is placed in a lake whose temperature is 63°C. Calculate the change in entropy of the cube-lake system as the ice cube comes to thermal equilibrium with the lake. The specific heat of ice is 2220 J/kg·K. (Hint: Will the ice cube affect the temperature of the lake?)
A 56 g ice cube at -31°C is placed in a lake whose temperature is 83°C. Calculate the change in entropy of the cube-lake system as the ice cube comes to thermal equilibrium with the lake. The specific heat of ice is 2220 J/kg·K. (Hint: Will the ice cube affect the temperature of the lake?)
10) A 100-g of ice at -10°C is placed in a lake whose temperature is 25°C. Calculate the change in entropy of the lake if we assume that the temperature of the lake does not change. (Cwater = 4190 J kg 'K'', Cice = 2220 J kg;'K.'; L; = 333 kJ kg;)
(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,...
A 250 g ice cube at -10∘C is placed in an aluminum cup whose initial temperature is 70∘C. The system comes to an equilibrium temperature of 20∘C.
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?
A 20.64 g ice cube at -1.93 oC is place in an aluminum cup whose initial temperature is 137.9 oC. The system comes to an equilibrium temperature of 17.96 oC. What is the mass in grams of the cup? The specific heat of ice is 2.093 J/g oC and that of aluminum is 0.901 J/g oC.
A 29.0 g ice cube at -15.0oC is placed in 180 g of water at 48.0oC. Find the final temperature of the system when equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter, i.e. the system is thermally insulated from the surroundings. Give your answer in oC with 3 significant figures. Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186 J/g K Latent heat of fusion for water: 333...