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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
How many joules are required for boiling 21.1g of water at 100C?
You need o know the initial temperature of water:Heat = specific heat x difference of temperature x mass of water
The average kinetic energy of water molecules is greatest in .?
Steam at 100C
Is the boiling of water at 100C and 1 atm a spontaneous process?
Yes, the boiling of water at 100C and 1 atm is a spontaneous process.
How many joules are required to raise 25 g of ice at 0C to steam at 100C?
Q = [ mI ] [ h sub sf + CshW ( 100.0 C - 0.0 C ) + h sub fg ]Q = [ 25 g ] [ 333.7 J /g + ( 4.184 J / g - C ) ( 100.0 C ) + 2257 J / g ]Q = [ 25 g ] [ 3009.1 J / g ] = 75230 J
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
If the heat of vaporization for water is 2260 Jg how many kilojoules are required to convert 5.00 g of liquid water at 100C to steam at 100C?
The heat required to vaporize 5.00 g of water is given by: 2260 J/g * 5.00 g = 11300 J. Converting this to kJ gives 11.3 kJ.
When do water molecules have the most greatest amount of energy?
Steam at 100C
How many joules are required for boiling 21.1g of water at 100C?
You need o know the initial temperature of water:Heat = specific heat x difference of temperature x mass of water
How much water is lost from 600ml when boiling at 100C for 20 seconds in a 2.5kW kettle?
No one can say, because that's not enough information. The more heat energy you provide, the faster the water will boil.If you provide exactly enough heat to keep the water at 100C, it won't boil at all!Every 540 calories of heat energy turns 1 gram of water to steam.600ml of water = 600 grams of water. So if you can provide 324,000 calories in 20 seconds - but I bet you can't! - you will turn all the water to steam.
What described water at 100 Celsius and 1 ATM pressure?
Water at 100°C and 1 atm pressure is in its liquid state, commonly referred to as boiling water. At this temperature and pressure, water reaches its boiling point and begins to vaporize into steam.
Why does steam at 100C damage the skin than water at 100C?
I think it's the other way - 100°C liquid water causes more damage than 100°C gaseous water. Liquid water has molecules that are much more densely packed than gaseous water. Since temperature is the measure of average kinetic energy, the molecules in liquid form move just as fast as the molecules in gaseous form. So if you stick your finger in liquid water, much more molecules will hit you. Unless that extra enthalpy of vaporization causes a difference in speeds of the molecules, then that extra energy required to vaporize water will be transferred to you, and you will feel more pain.
The average kinetic energy of water molecules is greatest in .?
Steam at 100C
Is the boiling of water at 100C and 1 atm a spontaneous process?
Yes, the boiling of water at 100C and 1 atm is a spontaneous process.
What is the pressure at the normal boiling of water?
100c
What temperateure does water boil?
212F or 100C
How many joules are required to raise 25 g of ice at 0C to steam at 100C?
Q = [ mI ] [ h sub sf + CshW ( 100.0 C - 0.0 C ) + h sub fg ]Q = [ 25 g ] [ 333.7 J /g + ( 4.184 J / g - C ) ( 100.0 C ) + 2257 J / g ]Q = [ 25 g ] [ 3009.1 J / g ] = 75230 J
