how much energy is required to raise the temperature of one liter of water 1o c?
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Quantifying Specific Heat Quantitative experiments show that 4.18 Joules of heat energy are required to raise the temperature of 1g of water by 1°C. Thus, a liter (1000g) of water that increased from 24 to 25°C has absorbed 4.18 J/g°C x 1000g x 1°C or 4180 Joules of energy.
824962
One liter of water is about 1 Kg or 1000g, giving Q = m x (delta T) x Specific heat of water = 1000g x 80C x 1 cal/g C= 80,000 cal or 80 Kcals. Technically, 80 kcals that is the amount of heat needed to get the liquid water to 100C and anything extra would go into vaporizing the water into steam.
486517
So about of heat required to change temperature is given by: H = mc∆T. (where m is mass in kg , c is specific heat and it's value is fixed . For water it is 4200J/kg ,for ice it is 2100 J/kg and for steam it is 2010J /kg.
809779
['A small calorie (cal) is the amount of energy required to raise the temperature of 1 gram (g) of water by 1º Celsius (º C).', 'A large calorie (kcal) is the amount of energy required to raise 1 kilogram (kg) of water by 1º C. It is also known as a kilocalorie.']
924713
It takes about 4200 J per liter/degree. Then you need to crystallize the water. It takes 333 KJ to cristallize 1 kg or 1 l of water (the density of water is 1). So in total you need to extract 417 KJ of energy.
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Quantitative experiments show that 4.18 Joules of heat energy are required to raise the temperature of 1g of water by 1°C. Thus, a liter (1000g) of water that increased from 24 to 25°C has absorbed 4.18 J/g°C x 1000g x 1°C or 4180 Joules of energy.
1210
1 cup of warm water (around 250ml) burns only about 12 calories.
963919
1 liter of water has a mass of 1 kg. If the water starts off at 100 degrees C, then the energy required to evaporate it would be 540,000 calories or 2.3 x 10^6 Joules.
1235500
To calculate the LHV you must subtract the heat of vaporization of H2O from the HHV. Long ago the heat of vaporization of water was 550 cal/g or (X the Mole wt of 18) 9900 cal/mole. Now it is (multiplying by 4.184 J/cal) 41,422J/mole or 41.4 kJ/mole (thanks to Mr. Metric).
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Answer: Water needs more energy to bring a change in its temperature as compared to soil.
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Quantitative experiments show that 4.18 Joules of heat energy are required to raise the temperature of 1g of water by 1°C.
389986
Phase changes in pure water occur at a specific temperature. At 1 atm, water freezes at 0° C and boils at 100° C. The energy required to change water from a liquid to a solid is 333.7 kJ/kg while the energy required to boil water is 2257 kJ/kg.
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Combining all the energy input totals, Gleick and Cooley found that producing bottled water requires between 5.6 and 10.2 million joules of energy per liter, depending on transportation factors (a typical personal-sized water bottle is about 0.5 liters).
334862
You have all heard of the BTU of heat energy (British Thermal Unit), it takes one BTU to raise one pound of water one degree Fahrenheit. So if the water in the pan on the stove is put in at 32°F, it will then require 180 BTU's to bring the water to boiling temperature, or 212°F.
419127
So in water it takes 1200 joule's to raise a Kg of water by 1 degree K or in degrees C. If this takes 1 min to boil the power required to boil the water equals 96kilo joules/60 seconds =1600 watts or 1.6 kilo watts.
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It takes 100 calories to heat 1 g. water from 0˚, the freezing point of water, to 100˚ C, the boiling point. However, 540 calories of energy are required to convert that 1 g of water at 100˚ C to 1 g of water vapor at 100˚ C. This is called the latent heat of vaporization.
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the standard molar heat of vaporization for water is 40.79 kJ/mol.