How much energy (in kJ) is released when 16.4 g of steam at 121.5 degrees C is condensed to give liquid water at 60.5 degrees C? The heat of vaporization of liquid water is 40.67 kJ/mol and the molar heat capacity is 75.3 J/(K*mol) for the liquid and 33.6 J?(K*mol) for the vapor.
"Energy is released when 100 kg of steam at 150 degrees Celsius and standard pressure changes to water at 60 degrees Celsius. Calculate the total energy change". I used q=mct to find the energy required to change to 100 degrees
1. How much heat energy is required to change 500 grams of water at 100 degrees Celsius to steam at 100 degrees Celsius? 2. How much energy is lost if 7kg of water is cooled from 46 degrees Celsius to 2 degrees Celsius? 3. How
How much thermal energy is released when 500g of steam at 100 degrees C condenses into liquid water and then cools to 50 degrees C? I tried to solve q=mct for q and then use that in the q=mLv formula but it didn't work. The answer
Please Help! I am having difficulties grasping these concepts. Explain please! 1. How much heat energy is required to change 500 grams of water at 100 degrees Celsius to steam at 100 degrees Celsius? 2. How much energy is lost if
How much thermal energy is released when 500 g of steam at 100 degrees celsius condenses into liquid and then cools to 50 degrees celsius. What I`ve Attempted: Q=mLv m = 500g (0.5 kg) Lv = 2.3*10^6 Q=(0.5)(2.3*10^6) Q=1,150,000 J