(15 points) An ice cube of mass 0.0340 kg and temperature -10.00 °C is placed in...
- -/10 points Thermo: Calorimetry - ice + steam 0/6 Submissions Used My Ne 0.1 kg of steam at 100°C is added to 0.41 kg of ice at 0°C. Determine the temperature of the mixture once thermal equilibrium is reached. 8. -70 points Specific Heats & Latent Heats 070 Submissions Used These values will be needed for the following calorimetry problems. SPECIFIC HEATS Specific Heat Substance (J/kg.K) Aluminum 900 Copper 390 Glycerin 2410 2100 Iron 450 Lead 130 Mercury 140...
Please answer 10, 11, and 12. 10. - 10 points Calorimetry: sub-zero ice cube to water 0/6 Submissions Used My Notes Ask Your Teacher room temperature of 20'C. The final situation A cube of ice is taken from the freewat-7.Candaced in a 10 g aluminum calorimeter filled with 3 is observed to be all water at what was the mass of the ice cube? 11. 10 points Calorimetry *2 06 Submissions Used My Notes Ask Your Teacher of water alised...
A 39 g ice cube at -69°C is placed in a lake whose temperature is 65°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?) Numbe UnitšT J/k the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Work
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?
We want to determine how much the room temperature increases when a kg of ice freezes.Suppose you have a freezer that needs 1 J of energy for every 3 J of heat it removes.How much thermal energy must be removed from 1 kg of water at room temperature? How much electrical energy is used to freeze the ice?What is the total energy, including waste heat, that is dumped into the kitchen? If the kitchen contains 40 kg of air, how...
A 0.07 kg ice cube at -300C is placed in 0.43 kg of 30.30C water in a very well-insulated container. What is the final temperature in degrees Celsius? Specific heat of ice = 2000 J/(kg.K), Specific heat of water = 4186 J/(kg.K), Latent heat of fusion of ice = 33.5 x 104 J/kg.
A 0.0600 kg ice cube at −30.0°C is placed in 0.537 kg of 35.0°C water in a very well insulated container. What is the final temperature? The latent heat of fusion of water is 79.8 kcal/kg, the specific heat of ice is 0.50 kcal/(kg · °C), and the specific heat of water is 1.00 kcal/(kg · °C).
Calculate the heat required to raise the temperature of gm of ice at -25˚C to 70˚C. (Ice has a specific heat of 2100 J/(kg K),the latent heat of fusion for ice is 334,000 J/kg, specific of water is 4186 J/(kg K) and Melting point of ice = 0˚C). Units are kJ.
An open container holds ice of mass 0.570 kg at a temperature of -18.0 ∘C . The mass of the container can be ignored. Heat is supplied to the container at the constant rate of 740 J/minute . The specific heat of ice to is 2100 J/kg⋅K and the heat of fusion for ice is 334×103J/kg. PART A: How much time tmelts passes before the ice starts to melt? PART B: From the time when the heating begins, how much...