156. The heat of vaporization of a certain refrigerant is 148 J/g. Calculate the number of...
32. An icemaker uses the heat change from evaporation of a refrigerant to freeze water. How many moles of the refrigerant CCI,F2 must be evaporated to freeze 209 g of water initially at 0°C to make ice at 0 °C? The heat of vaporization of CCI,F2 is 289 J/g. The heat of fusion of water is 334 J/g. A. 0.00 moles B. 1.00 moles C. 2.00 moles D. 3.00 moles E. 4.00 moles
The chlorofluorocarbon refrigerant Freon-12, CCl2F2, was banned in 1995 to help protect the ozone layer. Most new air conditioning units now use the re- frigerant tetrafluoroethane, CF3CH2F. The enthalpy of vaporization of Freon-12 is 155 Jg–1 and that of tet- rafluoroethane is 215.9 Jg–1. Estimate the number of grams of Freon-12 that must be vaporized to freeze a tray of 16 one-ounce (1 oz = 28 g) ice cubes with the water initially at 18°C. How many grams of tetrafluo-...
Using the heat of fusion for water 334 J/g the heat of
vaporization for water 2260 J / g and fhe specific heat of water
4.184 J/g C calculate the total amount of heat for each of the
following
Using the heat of fusion for water, 334 J/g. the heat of vaporication for water 2260 J/6, and the specific heat of water, 4 184J/g °C, calculate the total amount of heat for each of the following Part A joules released...
The heat of vaporization of water is 540 cal/g, and the heat of fusion is 80 cal/g. The heat capacity of liquid water is 1 cal g−1 °C−1, and the heat capacity of ice is 0.5 cal g−1 °C−1. 18 g of ice at -6°C is heated until it becomes liquid water at 40°C. How much heat was required for this to occur?
The latent heat of vaporization of H2O at body temperature (37.0 °C) is 2.37E+6 J/kg. To cool the body of a 77.9 kg jogger [average specific heat capacity = 3450 J/(kg·°C)] by 1.70 °C, how many kilograms of water in the form of sweat have to be evaporated?
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.
The latent heat of vaporization of H2O at body temperature (37.0°C) is 2.37E+6 J/kg. To cool the body of a 74.6 kg jogger [average specific heat capacity = 3480 J/(kg*°C)] by 1.20°C, how many kilograms of water in the form of sweat have to be evaporated?
The latent heat of vaporization of H2O at body temperature (37.0°C) is 2.39E+6 J/kg. To cool the body of a 72.6 kg jogger [average specific heat capacity = 3530 J/(kg*°C)] by 1.10°C, how many kilograms of water in the form of sweat have to be evaporated?
4-10. The latent heat of fusion of ice is 333 kJ/kg. In the freezer compartment of a refrigerator, a tray holds 12 cubes of water each of mass 8.0 g. If the C.O.P. of the refrigerator is 3.3. how many kilowatt-hours of electrical energy would be required to run the refrigerator to change the water cubes (at 0°C) into ice cubes (at 0°C)?
heat capacity of ?2?(?) 37.7 J/(mol⋅K) heat capacity of ?2?(?) 75.3 J/(mol⋅K) enthalpy of fusion of ?2? 6.01 kJ/mol Two 20.0‑g ice cubes at −14.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.