Soda from a mS = 12 oz can at temperature TS = 10.5°C is poured in its entirety into a glass containing a mass mI = 0.19 kg amount of ice at temperature TI = -16.5°C. Assume that ice and water have the following specific heats: cI = 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 can assume that 1 kg of either soda or water corresponds to 35.273 oz. a. In degrees Celsius, what is the final temperature Tfinal of the mixture?  b. Write an expression for how much of the ice mmelted has melted.  c. In kilograms, how much of the ice mmelted has melted?

Specific heat (c) J/kg C 900 Problem 6: Consider a 0.775 kg aluminum pot containing 2.35 kg of water. Substances Solids Aluminum kcal/kg-C 0.215 Concrete 840 0.20 Copper 387 0.0924 Glass 840 0.20 Human Body (37°C) 3500 0.83 Iron, steel 452 0.108 Liquids Water 4186 1.000 Mercury 139 0.0333 Part (a) How much heat, in kilocalories, must be transferred to raise the temperature of the aluminum pot and the water from 30.0°C to the boiling point of water and then boil away 0.775 kg of water (L, = 539 kcal/kg)? Q = sin() cos() tan() 7 8 9 HOME cotan() asin() acos() E 6. atan() acotan() sinh() 1 2. 3 cosh() tanh() cotanh() + END ODegrees O Radians Vol BACKSPACE DEL CLEAR Feedback I give up! Submit Hint Part (b) How long, in seconds, does this take if the rate of heat transfer is 500 W?

Water with a mass of mW = 0.400 kg and temperature of TW = 18.5°C is poured into an insulated bucket containing mI = 0.11 kg of ice at a temperature of TI = -18°C. Assume the specific heats of ice and water are constant at cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively. The latent heat of fusion for water is Lf = 334×103 J/kg. What is the final temperature of the mixture, in degrees Celsius?

How much thermal energy/heat is required to raise 2.3 kg of lead from 300°C to 1800°C? Use Table 1 p281 and Table 1 p291 to help you. O 1.8 x 10°J O 2. 5 x 10°J O8.2 x 10³J O4.5 x 10°J x 10°J