A 1.3kg block of ice at -30 C is placed in thermal contact with a 7kg piece of al at 280 C. Determine how much ice melts and its final temperature?
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A 1.3kg block of ice at -30 C is placed in thermal contact with a 7kg piece of al at 280 C. Determine how much ice melts and its final temperature?
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- Soda from a mS = 12 oz can at temperature TS = 20.5°C is poured in its entirety into a glass containing a mass mI = 0.16 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?A 0.012 kg cube of ice at 0.0°C is added to 0.477 kg of soup at 81.7°C. Assuming that the soup has the same specific heat capacity as water, find the fi- nal temperature of the soup after the ice has melted. The specific heat of water is 4186 J/kg °C and water's latent heat of fu- sion is 3.33 x 105 J/kg. Answer in units of °C. Your response... Previous Responses X #1.79.7 PALETTEA stone of mass 13 kg is dropped into a tank of water from just above the watersurface. The tank contains 100kg of water which is 1.3m deep. The stone has aspecific heat of 1000 J/kgK and water 4200 J/kgK. If the water and stone are initiallyat the same temperature, determine the temperature rise f the water. State anyassumptions made answer: 3.8x10^-4K
- Please asapA 23 g ice cube at -15.0oC is placed in 129 g of water at 48.0oC. The Specific heat of ice is 2.090 J/g K, the specific heat of water is 4.186 J/g K, and the latent heat of fusion for water is 333 J/g. What is final temperature in celsius of the system when the equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter.Ice has formed on a shallow pond, and a steady state has been reached, with the air above the ice at -7.6°C and the bottom of the pond at 3.7°C. If the total depth of ice + water is 2.3 m, how thick is the ice? (Assume that the thermal conductivities of ice and water are 0.40 and 0.12 cal/m-Cº-s, respectively.) Number Units
- Your 500 cm3 soda is at 20° C so you add 100 g of ice which is at –20° C. Does all the ice melt? If so, what is the final temperature? If not, what fraction of the ice melts? Assume the cup is well–insulated and that the soda has the same thermal properties as liquid water.a cup of coffee sits on a table in an insulated mug. to coool the coffee down a ice block is added. the inital mass of coffee in the mug is 90g. the intial temperature of the coffee is 90 degree celsius. the ice block has started to melt and is then put into the coffee. the ice melts and the new temperature of the cofee is 78 degree c and the new mass is 110g. the ice block (final-intital mass) is 20g. what are teh tempeartuare changes for the coffee and ice (started at 0 degree celsius) also if specific heat of water is used for both the coffee and ice waht is the heat energy lost by the coffee and the heat energy gained by the ice after it melted?