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How many calories are needed to change 10 grams of ice at 0 degree to steam at 100 degree Celsius?
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- An ice tray is removed from a freezer, where the ice was at a temperature of -11°C, and left on a countertop. If the mass of the ice is 0.29 kg, how much heat must be added in k to turn all the ice into room temperature water (that is, liquid water at 20°C)? The specific heat of water is 4.2 kgC kJ the heat of fusion of water is 335 kg kJ and the specific heat of ice is 2.1 kg°C* 133.69 This is a change of phase question. There are 3 cases we have to consider: 1. The heat required to increase the temperature of the ice, Q1 2. The heat required to turn the ice into a liquid (a phase change), Q2 3. The heat required to raise the temperature of the now liquid water, Q3 For Q1, you will use the equation Q = mcATusing the c=2.1 kJ/(kg*C). Keep in mind that the hpA 75-kg block of ice at -13°C is placed in an oven set to a temperature of 105°C. The ice eventually vaporizes and the system reaches equilibrium. How much energy, in joules, is needed to vaporize all the water at 100°C? How much energy, in joules, is required to heat the resulting steam from 100°C to 105°C? What is the total energy, in joules, that is needed to heat the block of ice from its initial temperature to water vapor at its final temperature?How many joules are needed to change 50g of ice at 0°C to steam at 120°C?The latent heat of fusion of ice is 3.35 x 10°J/kg; latent heat of vaporization of water is 2.26 x 10°J/kg. The specific heat capacities of ice; water, and steam, respectively, are 2093 J/(kg. K), 4186 J/(kg. K) and 2010 J/(kg. K). out of Select one: A. 50.68 kJ B. 63.96 kJ O C. 227.6 kJ D. 53.96 kJ E. 20.5 kJ F. 800.2 kJ G. 153.7 kJ H. 22.76 kJ
- A student measures the following data in a calorim- etry experiment designed to determine the specific heat of aluminum: Initial temperature of water 70.0°C and calorimeter: 0.400 kg Mass of water: 0.040 kg Mass of calorimeter: Specific heat of calorimeter: 0.63 kJ/kg · °C 27.0°C Initial temperature of aluminum: 0.200 kg Mass of aluminum: Final temperature of mixture: 66.3°C Use these data to determine the specific heat of aluminum. Explain whether your result is within 15% of the value listed in Table 11.1.The number of kilocalories in food is determined by calorimetry techniques in which the food is burned and the amount of heat transfer is measured. How many kilocalories per gram are there in a 4.9-g peanut if the energy from burning it is transferred to 0.48 kg of water held in a 0.095-kg aluminum cup, causing a 54.9degree celsius temperature increase?An ice tray is removed from a freezer, where the ice was at a temperature of -12°C, and left on a countertop. If the mass of the ice is 0.35 kg, how much heat must be added in kJ to turn all the ice into room temperature water (that is, liquid water at 20°C)? The specific heat of water is 4.2 kg°C kJ the heat of fusion of water is 335 , and the specific heat of ice is 2.1 kg°C kJ
- When air is inhaled, it quickly becomes saturated with water vapor as it passes through the moist upper airways. When a person breathes dry air, about 25 mg of water are exhaled with each breath. At 12 breaths/min, what is the rate of energy loss due to evaporation? Express your answer in both watts and Calories per day. At body temperature, the heat of vaporization ofwater is Lv = 24 × 105 J/kg.How much heat do you need to remove from 2 g of steam at 100oC to convert it to water at 100oC?Assume atmospheric pressure. Answer is in the unit of calories.An ice cube tray of negligible mass contains 0.350 kg of water at 18.0 degree How much heat must be removed to cool the water to 0.0 degree C and freeze it? Express your answer in joules, calories and Btu.
- A 0.045-kg ice cube at -30.0°C is placed in 0.405 kg of 35.0°C water in a very well-insulated container. The latent heat of fusion for water is Lf = 79.8 kcal/kg. What is the final temperature of the water, in degrees Celsius? Tf =AsapEthyl alcohol has a boiling point of 78.0°C, a freezing point of -114 °C, a heat of vaporization of 879 kJ/kg, a heat of fusion of 109 kJ/kg, and a specific heat of 2.43 kJ/kg-K. How much energy must be removed from 0.510 kg of ethyl alcohol that is initially a gas at 78.0 °C so that it becomes a solid at -114 °C?