(0%) Problem 4: Soda from a ms= 12 oz can at temperature Ts = 11.5°C is...
(20%) Problem 2: A piece of unknown material has a mass of m, = 0.79 kg and an initial temperature of Tu = 79°C. The specific heat of water is cw = 4.180 x 102 J/(kg:°C). 50% Part (a) The sample of material is dropped into my = 1.4 kg of water at T = 19°C in a calorimeter. The calorimeter reaches a final temperature of Te = 34°C. Enter an expression for the specific heat of the unknown material,...
IIVIT ILI I ILUDLSU DL. U ZUI12.01.UUIII DUDULL. 11/21/2011.J.UUI1I LUDU. 12/UZUI11.J.UUI11 (0%) Problem 4: Soda from a m3= 12 oz can at temperature Tg = 15°C is poured in its entirety into a glass containing a mass mī= 0.13 kg amount of ice at temperature T,= -15.5°C. Assume that ice and water have the following specific heats: 0,= 2090 J/(kg.°C) and cs= 4186 J/(kg.°C), and the latent heat of fusion of ice is Lf= 334 kJ/kg. In this problem you...
A 82 g cube of ice at 0°C is dropped into 1.0 kg of water that was originally at 80°C. What is the final temperature of the water after the ice has melted? The specific heat of ice is 2090 J/kg°C, and the latent heat of fusion of ice is 3.33x105 J/kg.
How much heat must be removed from 456 g of water at 25.0 degree C to change it into ice at -10.0 degree C? The specific heat of ice is 2090 J/kg K. the latent heat of fusion of water is 33.5 times 10^4 J/Kg, and the specific heat of water is 4186 J/kg K.
A 25.0-g block of ice at -15.00°C is dropped into a calorimeter (of negligible heat capacity) containing water at 15.00°C. When equilibrium is reached, the final temperature is 8.00°C. How much water did the calorimeter contain initially? The specific heat of ice is 2090 J/kg ∙ K, that of water is 4186 J/kg ∙ K, and the latent heat of fusion of water is 33.5 × 104 J/kg.
How much heat is required to change 456 g of ice at -20.0Degree C into water at 25.0Degree C? specific heat of water = 4186]/(kg-K); specific heat of ice = 2090 J/(kg.K) and latent heat of fusion of water = 33.5 times 10^4 J/kg.
2. How much heat transfer is necessary to raise the temperature of a 0.500 kg piece of ice from -30.0C to 110.0 C? cice-2090 J/kg C, Cater 4186 J/kg C,Cseam 1520 J/kg C, L-334 kJ/kg and Lv-2256 kJ/kg. 2. How much heat transfer is necessary to raise the temperature of a 0.500 kg piece of ice from -30.0C to 110.0 C? cice-2090 J/kg C, Cater 4186 J/kg C,Cseam 1520 J/kg C, L-334 kJ/kg and Lv-2256 kJ/kg.
The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at 0 °C is added to it. The desired final temperature of the water is 11 °C. The latent heat of fusion for water is 33.5 × 104 J/kg, and the specific heat capacity of water is 4186 J/(kg·C°). Ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added.
The temperature of 2.7 kg of water is 34° C. To cool the water, ice at 0° C is added to it. The desired final temperature of the water is 11° C. The latent heat of fusion for water is 333.5 × 103 J/kg, and the specific heat capacity of water is 4186 J/(kg·C°). Ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added. m = kg
A 26 g block of ice is cooled to −62 ◦C. It is added to 569 g of water in an 80 g copper calorimeter at a temperature of 27◦C. Find the final temperature. The specific heat of copper is 387 J/kg · ◦C and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer in units of ◦C.