Wiki User
∙ 11y agoAssuming standard atmospheric pressure, 2260 kilojoules.
Wiki User
∙ 11y agoLeaving aside the effects of pressure, yes, the temperatures are the same. But the amount of heat (thermal energy) per gram, is much greater for the steam.
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.
6,520 Btus
This is the latent heat of vaporisation of water, which at standard pressure, is 539 calories (per gram).
All calculations below are assumed done with all materials (ice, water, and steam) being at normal atmospheric pressure. 3.0kg is 3000 gm. Heat required to raise temperature of ice from -10 degree celcius to 0 degrees celcius is 3000 x 10 cals. (A) The latent heat of fusion of ice is 80 cals per gm. So heat needed to melt 3000 gm of ice at 0 degrees celcius is 3000 x 80 cal. (B) The heat required to convert 3000 gms of water from 0 degrees celcius to 100 degrees celcius is 3000 x 100 cals. (C) The latent heat of vaporization of steam is approximately 540 cals per gm. Hence heat required to convert 3000 gms of water to steam at 100 degrees celcius is 3000 x 540 cals. (D) Now add (A) + (B) + (C) + (D) = 30000 + 240000 + 300000 + 1620000 cals. And that is = 2190000 cals = 2.19 X 10 to power 6 cals.
To convert 12.5 grams of ice at 0 degrees Celsius to steam at 100 degrees Celsius, you would need to provide heat energy for three main processes: heating the ice from 0 degrees Celsius to 100 degrees Celsius, melting the ice into water at 0 degrees Celsius, and then heating the water from 0 degrees Celsius to steam at 100 degrees Celsius. The total calorie requirement would be determined by the specific heat capacities and heat of fusion and vaporization of water.
To convert 4 kg of ice at 0 degrees Celsius to steam at 100 degrees Celsius, you would need to calculate the heat required to raise the temperature of ice to 0 degrees Celsius, melt the ice to water at 0 degrees Celsius, raise the temperature of water to 100 degrees Celsius, and then convert water to steam at 100 degrees Celsius. The total amount of heat needed can be calculated using the specific heat capacities and latent heats of fusion and vaporization of water.
No, steam cannot be hotter than 100 degrees Celsius. At this temperature, water is converted into steam and any additional heat added will not increase the temperature, but will only convert more water into steam.
The steam point of the Celsius scale is 100 degrees Celsius. At this temperature, water boils and turns into steam.
The amount of heat required to convert 1 kg of steam to water at its boiling point is known as the latent heat of vaporization. For water, this amount is approximately 2260 kJ/kg.
Water changes into steam or water vapor above 100 degrees Celsius.
At 105 degrees Celsius, steam will remain in the gaseous phase as it is above the boiling point of water (100 degrees Celsius). Steam will continue to condense into liquid water only once it cools down below the boiling point.
If you heat steam above 100 degrees Celsius, it will continue to increase in temperature without changing to water. This is because steam is already in a gaseous state at temperatures above 100 degrees Celsius.
Water becomes steam at 100 degrees Celsius under normal atmospheric pressure.
It equals one kilpod.
It can be anywhere in between 60C and 100C (boiling point).
Steam is usually at a temperature of 212 degrees Fahrenheit (100 degrees Celsius) when it forms at sea level.