I have the data but I am having a hard time determining the end result.
How much heat energy is required to raise the temp. of 5.0g of H20 from -10C to 110C ? (ice to steam)
Given the following data:
Specific Heat J/gK Molar Heat Capacity J/molK Formula Mass
Water (l) 4.184 75.3 18.0
Ice 2.05 36.9 18.0
Water Vapor 1.84 33.1 18.0
This solution is provided in 181 words. It demonstrates through five steps, including heating, melting, heating again, boiling, and heating the steam, how much total heat energy is required.
... If 0.534 of room-temperature water is heating on the stove, how many kilojoules of heat energy have been absorbed by the water at the moment it begins to boil? ...
... When still more heat is present, the molecules have enough energy to break free of even the hydrogen bonds and water molecules escape to a gaseous state where ...
... 4. To change the phase at 1000C form liquid to vapour ie from water to steam The amount of energy required Q4 is given by Q4 = mass*latent heat of vaporization ...
... A supply of geothermal hot water is to be used as the energy source in an ... of 85°C, and the condenser temperature is 40°C. Calculate the heat transfers in ...
...heat energy after mixing the cold and hot water? ... You can calculate the calorimeter heat energy as the ... between the initial and final heat energies.Choose the ...
... Amount of energy produced by burning 500 mol C5H12: 0.6262*500/(72*2 ... 14256.052 kJ>2445.67883 kJ, we have sufficient pentane to heat up the pot and water. ...
... is then 3.5527025 KJ where I multiplied the temperature difference by the heat capacity of the mass of water. This change in energy is the heat capacity of the ...
... flowing at niagra falls in new york drops 96.3 meters if all the energy of the water falling is converted to heat how much heat energy would the water have. ...
... 1 degree C is 4.18 J. Thus, the specific heat capacity of water is 4.18 J / °C g and energy gained or lost by a certain amount of water is calculated by: s X ...
