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What is the thermal energy needed to completely vaporize 18.02g of water at 100 degrees?
To calculate the amount of energy require to vaporise water at 100C
You need to first find the Latent heat of Vaporisation which for water is
2260kJ/kg
So to find the amount of energy required you merely multiply the mass of the water in kg by 2260.
Density of water is more or less 1kg per litre at room temperature however at 100C it could be less
What else can I help you with?
What type of energy is required to begin the distilling process?
The thermal energy is needed.
What term describes the amount of thermal energy that is required to raise the temperature of a substance by 1.0 degrees Celsius?
Specific heat capacity is the term that describes the amount of thermal energy required to raise the temperature of a substance by 1.0 degree Celsius.
How much energy is required to vaporize 1.5 of aluminum?
1650kj
How much is required to vaporize 2 kg of copper?
9460 kJ
How many calories are needed to vaporize 1 gram of boiling water at 100 degrees?
To vaporize 1 gram of boiling water at 100 degrees Celsius, it would require approximately 2260 joules, which is equivalent to about 0.54 calories. This energy is needed to break the intermolecular bonds holding water molecules together, allowing them to escape into the gas phase.
What is meant by saturated liquid vapor?
Any addition of thermal energy to a saturated liquid will cause it to vaporize. Any subtraction of thermal energy from a saturated vapor will cause it to condense.
How do the states of matter change based on thermal energy?
They melt (liquefy), freeze (solidify), vaporize, or condense.
Is degrees related to thermal energy?
The amount of thermal energy a substance has is proportional to its temperature
Would thermal energy be greater at 0 degrees Celsius or 48 degrees Fahrenheit?
Thermal energy is a measure of the internal energy of a system and is not dependent on the unit of temperature used. Therefore, the thermal energy at 0 degrees Celsius would be the same as at 48 degrees Fahrenheit.
How much thermal energy is necessary to vaporize 36.000 g of water at its boiling point?
To calculate the thermal energy required to vaporize water, we use the formula: ( Q = m \times L_v ), where ( m ) is the mass of the water and ( L_v ) is the latent heat of vaporization of water, approximately 2260 J/g. For 36,000 g of water, the thermal energy needed would be ( Q = 36,000 , \text{g} \times 2260 , \text{J/g} ), which equals 81,360,000 J, or 81.36 MJ. Thus, 81.36 megajoules of thermal energy is necessary to vaporize 36,000 g of water at its boiling point.
Why do you loose thermal energy if your body temperature is 37 degrees c and the temperature around you is 25 degrees c?
Because thermal energy travels from hotter objects to colder objects.
Does gold conducts thermal energy?
More or less everything conducts thermal energy, but to different degrees.
Explain whether your body gains or loses thermal energy if your body temperature is 37 degrees Celsius and the temperature around you is 25 degrees Celsius?
25degres celsius has more thermal energy
What is the thermal energy needed to completely melt 9.60 mol of ice at 0.0 degrees celsius?
Anything hotter than 0 degrees that radiates heat.
Does your body gain or lose thermal energy if your body temperature is 37 degrees Celsius and the temperature around you is 25 degrees Celsius?
You will lose thermal energy.Heat (energy) will always flow from warmer to cooler.
What has more thermal energy a bath tub at 45 degrees or a cup of coffee at 90 degrees?
Bathtub at 45 degrees
Explain whether your body gains or loses thermal energy if your body temp is 37 degrees Celsius and then temp around you is 25 degrees Celsius?
Your body would gain thermal energy because thermal energy only moves from something at a higher temperature to something at a lower temperature.
