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That completely depends on how much steam there is. (mass)
Approx 2940 Joules.
539 calories per gram for heat of vaporization plus 1 cal/gram/degree C 100 degrees C - 80 degrees C = 20 degrees C (539 calories + 20 calories) X 50 kg X 1000 gm/kg = 27950000 cal = 27,950 kcal
ACCORDING TO PHYSICS :- Since the latent heat of vaporisation of Steam is so high as 2268 Joules , thus so as to convert from the Gaseous State to liquid Sate , Steam liberates 2268 J/Kg of heat energy to the Surrounding. In this way it proves more efficient to use Steam than Electricity for heating.
No. it is an energy repository. Fuels of various kinds are used to heat water into steam. the steam has more energy than the water.
That completely depends on how much steam there is. (mass)
Approx 2940 Joules.
Use this formula. q(in Joules) = Mass * specific heat * change in temperature I will use specific heat of water at 25 C. You can look up specific heat of steam. You say " heat to " so I assume you have final and initial heat backwards. q = 25.0 grams H2O * 4.180 J/gC * (100.0 C - 29.25 C ) q = 7393 Joules
A 300 grams of water takes about 90 seconds to boil in a 2 kW kettle, so that is 2000 watts x 90 seconds which is 180,000 Joules of energy. But to convert that water completely into steam requires an extra 300x550x4.2 Joules, which is nearly 700,000 Joules. So converting it to steam takes 4-5 times as much energy as boiling it. That is why it takes a while for a kettle to boil dry.
Assuming the water is liquid, the specific heat is about 4.186 joule/gram·°C, so to heat 46 grams of water would take about 192.556 joules/°C. The specific heat of ice is about 2.100 Joules/g·°C so heating 46 g of frozen water would take about 96.6 joules/°C. The specific heat of steam is about 2.020 Joules/g·°C so heating 46 g of water vapor would take about 92.2 joules/°C.
You mean how much heat energy will be lost/transferred as you are losing Joules here. All in steam, so a simple q problem and no change of state. 2.67 kg = 2670 grams q = (2670 grams steam)(2.0 J/gC)(105 C - 282 C) = - 9.45 X 105 Joules ----------------------------------- This much heat energy must be lost to lower the temperature of the steam.
inside steam is tiny particals that is called steam energy this steam energy are a type of energy used in factorys
Yes. Steam is an example of thermal energy.
539 calories per gram for heat of vaporization plus 1 cal/gram/degree C 100 degrees C - 80 degrees C = 20 degrees C (539 calories + 20 calories) X 50 kg X 1000 gm/kg = 27950000 cal = 27,950 kcal
ACCORDING TO PHYSICS :- Since the latent heat of vaporisation of Steam is so high as 2268 Joules , thus so as to convert from the Gaseous State to liquid Sate , Steam liberates 2268 J/Kg of heat energy to the Surrounding. In this way it proves more efficient to use Steam than Electricity for heating.
As the steam comes in contact with the skin, it becomes water, and releases more energy (about 2188 joules per gram) on contact than water at the same temperature.
While some forms of energy can be considered as either particle or wave, steam is not one of those. The energy of steam comes from it expansion. There is no steam energy particle.