20 kg of steam at 383 K transfers Q = 1.5 × 106 J of its energy to the environment. What is the mass of water that condenses? (The latent heat of fusion is Lf = 3.3 × 105 (J/kg) and the latent heat of vaporization is Lv = 2.26 × 106 (J/kg). The specific heat of steam is csteam = 2010 (J/(kg ◦C) and cwater = 4186 (J/(kg ◦C).) A) 0.0 kg B) 0.5 kg C) 7.2 kg D)...
QUESTION 8 Heat has to be withdrawn from 100 g steam at 110 °C to convert into water at 20 °C. The amount of heat needed to withdraw will be { GIVEN CONSTANTS: Specific Heat of Water = 4186 J/kg ºc, Specific Heat of Steam = 2013 J/kg ºc, Spedific Heat of Steel = 452.1 J/kg ºc, Specific Heat of Copper = 385.1 J/kg ºc, Latent Heat of Vaporization = 2.26 x 106J/kg. } 0 251500 J 26100 J 0...
Calculate the final equilibrium temperature when 10.0 grams of steam initially at 100 degree C is mixed with 450 grams of liquid water and 110 grams of ice at 0 degree C in a calorimeter. That is, the liquid water AND the ice are initially at 0 degree C. Ignore any heat energy exchanges with the calorimeter and the surroundings. If you conclude that the final temperature of the system is 0 degree C, then what mass of ice remains,...
You have a container holding 45 grams of water at 25.0 °C and 750-gram block of aluminum. Your goal is to heat the aluminum block so that it boils all of the water away when placed in the container. What minimum temperature is needed? Consider the water + aluminum to be an isolated system (i.e., ignore any heat flow to the environment, which includes the container). The specific heats of aluminum and water are 900.0 and 4186 J/kg°C respectively. The...
An 825 g iron block is heated to 352°C and placed in an insulated container (of negligible heat capacity) containing 40.0 g of water at 20.0°C. The following may be useful: specific heat of water = 4186 J/(kg K); specific heat of water vapor = 2090 J/(kg K); specific heat of iron = 560 J/(kg K); latent heat of vaporization for water = 2.26 x 106 J/kg. a. Is the final temperature less than, equal to, or larger than 100°C?...
An 825 g iron block is heated to 352°C and placed in an insulated container (of negligible heat capacity) containing 40.0 g of water at 20.0°C. The following may be useful: specific heat of water = 4186 J/(kg K); specific heat of water vapor = 2090 J/(kg K); specific heat of iron = 560 J/(kg K); latent heat of vaporization for water = 2.26 x 106 J/kg. Is the final temperature less than, equal to, or larger than 100°C? You...
How much energy is required to change a 47 g ice cube from ice at -12 C to steam at 117°C? The specific heat of ice is 2090 J/kg. C, the splecific heat of water is 4186 J/kg C, the specific heat of stream is 2010 J/kg. C, the heat of fusion is 3.33 x 105 J/kg, and the heat of vaporization is 2.26 x 106 J/kg Answer in units of J
A quantity of frozen water (also called ice) of mass 0.0360 kg is initially at a temperature of -4.000 C. It undergoes a series of physical changes at atmospheric pressure. The specific heat of ice is 2090 J/kg.°C The specific heat of water is 4186 J/kg.°C The specific heat of steam is 2010 J/kg.°C. The heat of fusion of water is 3.33 105 J/kg. The heat of vaporization of water is 2.26 106 J/kg. (a) Calculate the amount of heat...
014 10.0 points How much energy is required to change a 35 g ice cube from ice at -12°C to steam at 111°C? The specific heat of ice is 2090 J/kg.° C, the specific heat of water is 4186 J/kg.° C, the specific heat of stream is 2010 J/kg.° C, the heat of fusion is 3.33 x 10° J/kg, and the heat of vaporization is 2.26 × 106 J/kg. Answer in units of J
ADDITIONAL PROBLEMS Question 11.1a: A sealed container isolated from its environment holds 0.730-kg of water at 15.5°C. A heater inside the container delivers 4.50 x 105 J of energy to the water. Neglect any energy transferred to or from the container. Water boils at 1.00 x 102°C, has specific heat of 4.19 x 103 J/(kg °c), and a latent heat of vaporization of 2.26 x 106 J/kg. Determine the mass of water converted to steam. kg Need Help? Read