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To determine the heat released, you need to calculate the heat lost during the cooling process. First, calculate the heat lost when steam at 100°C condenses to water at 100°C. Use the formula Q = m * c * ∆T, where m is the mass, c is the specific heat capacity, and ∆T is the temperature change. Then, calculate the heat lost when water at 0°C freezes to ice at -15°C using the same formula. Finally, add the two calculated values to find the total heat released.
What else can I help you with?
How much heat in joules is released when 1000 g of steam at 100 C condenses to water at the same temperature?
To calculate the heat released when 1000 g of steam at 100°C condenses to water at the same temperature, we use the latent heat of vaporization for water, which is approximately 2260 J/g. Therefore, the heat released can be calculated as follows: Heat released = mass × latent heat of vaporization = 1000 g × 2260 J/g = 2,260,000 J. Thus, 2,260,000 joules of heat is released during the condensation process.
How much heat must be transferred for 20 g of liquid water at 100 C to become steam is it absorbed or released?
The heat required to convert 20 g of liquid water at 100°C to steam at 100°C is the heat of vaporization of water. This is 2260 J/g. Therefore, the total heat required is 20 g * 2260 J/g = 45200 J. This amount of heat is absorbed by the water as it changes phase from liquid to steam.
Which has higher temperature steam or water boling in kettle?
Steam. The reason for this is water boils at the temperature of 212 degrees F. Steam can be heated to much higher temperatures than that. Some engines that are water cooled has steam at temperatures of over 700 degrees. Water basically becomes a plasma at this temperature.
A quantity of steam at 110 C is condensed and the resulting water is frozen into ice at 0 C. How much heat was removed?
The amount of heat removed during the process of steam condensing and then freezing into ice is calculated by adding the heat required to condense the steam and the heat required to freeze the resulting water. This is determined using the specific heat capacity and latent heat of vaporization/condensation for water.
How many joules of energy are necessary to heat the steam from 100.0 degree c to 114.0 degree c?
To calculate the energy required to heat a substance, you can use the formula: Q = mcΔT, where Q is the heat energy, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature. You will need to know the specific heat capacity of steam to determine the energy required to heat it.
How much heat is released when 160 grams of steam at 100 degrees C liquefies?
The heat released when steam at 100 degrees Celsius condenses into liquid water is equal to the heat it absorbed during the phase change from liquid water to steam. This heat is known as the latent heat of vaporization, which for water is approximately 2260 J/g. Therefore, the amount of heat released when 160 grams of steam liquefies is approximately 160g x 2260 J/g = 361,600 J.
Why is heat trasnfer coefficient of saturated steam is higher than superheated steam?
when steam is at its saturation point for a given pressure, any heat removed will cause liquid water to form. So when saturated steam is used to heat something else, the heated object/substance receives the condensation heat of the steam. The latent heat of condensation/evaporation is 970 But/lb @ 0 psig. On the other, superheated steam only gives up about 10 BTU/lb if it is cooled 20 degrees F. That means that much more steam would be used to transfer the equivalent amount of heat. The liquid water interface also improves the heat transfer.
How much heat is released when 1000g of steam at 100 degrees Celsius condenses?
When steam at 100 degrees Celsius condenses, it releases 2260 Joules of energy per gram. Therefore, for 1000g of steam, the heat released would be 2,260,000 Joules (2260 J/g * 1000 g).
How much heat in joules is released when 1000 g of steam at 100 C condenses to water at the same temperature?
To calculate the heat released when 1000 g of steam at 100°C condenses to water at the same temperature, we use the latent heat of vaporization for water, which is approximately 2260 J/g. Therefore, the heat released can be calculated as follows: Heat released = mass × latent heat of vaporization = 1000 g × 2260 J/g = 2,260,000 J. Thus, 2,260,000 joules of heat is released during the condensation process.
How much heat is released when 12.4 g of steam at 100 degrees celsius condenses to water at 100 degrees celsius?
The latent heat of condensation of steam is 2260 Joules per gram (539.3 cals/g). So the amount of heat released by 12.4 g = 12.4*2260 Joules = 28,024 Joules or 6687 cals.
How much heat must be transferred for 20 g of liquid water at 100 C to become steam is it absorbed or released?
The heat required to convert 20 g of liquid water at 100°C to steam at 100°C is the heat of vaporization of water. This is 2260 J/g. Therefore, the total heat required is 20 g * 2260 J/g = 45200 J. This amount of heat is absorbed by the water as it changes phase from liquid to steam.
How much steam is made on a Navy ship?
It depends on the ship in question. Steam is often used for things other than just propulsion. It is sometime used to heat a ship and to heat hot water. Nuclear and steam vessels run their power on steam.
Fifty grams of water cooled from 50 degrees to 10 degrees if the specific heat of wayer is 4.2 hoe much was released?
The amount of heat released can be calculated using the formula: Q = mcΔT, where Q is the heat released, m is the mass (50g), c is the specific heat (4.2 J/g°C for water), and ΔT is the change in temperature (50°C - 10°C). Substituting the values, we get Q = 50g * 4.2 J/g°C * (50°C - 10°C) = 8400 J (or 8.4 kJ) of heat released.
When 30 grams of water is converted into steam how much heat is absorbed?
q = mHvq = heatm = mass (30g)Hv = heat of vaporization (2,260J/g)q = (30g)(2,260J/g)q = 67,800JWhen 30 grams of water is converted into steam, how much heat is absorbed?67,800J of heat, also represented as 67.8kJ of heat is absorbed.
Why the water cooled condensers have to be used in the water steam cycle of power plant?
Some of the heat is used to produce electricity, the rest is waste and put into the environment. Much of the energy of the heat is lost as the steam passes through the turbines, with the heat being converted to mechanical energy, and then to electrical. This accounts for about 35% to 40% of the energy of the heat, cooling it by the removal of that heat. It would be possible for residual heat to be tapped for conversion into electricity, also, but this is not done in most nuclear reactors. Converting it to electricity would get another 10% or so of the heat of the remaining steam, cooling the steam further. The remainder of the heat is waste. It is dumped into the environment, primarily into the air, by using heat exchangers and cooling towers. In this system, the steam is used to heat water, condensing in the process. The water is then used to heat air in the cooling tower. Another way to get rid of waste heat is to use heat exchangers to heat a nearby body of water, such as a lake, the ocean, or a river. This is usually done only in the summer, when the atmosphere is warm and the cooling towers are not efficient enough to do their work.
Which has higher temperature steam or water boling in kettle?
Steam. The reason for this is water boils at the temperature of 212 degrees F. Steam can be heated to much higher temperatures than that. Some engines that are water cooled has steam at temperatures of over 700 degrees. Water basically becomes a plasma at this temperature.
What is meant by wet and dry steam?
Dry steam is superheated , meaning more heat has been added resulting in no liquid phase present and the heat of vaporazation has been surpassed adding to the total enthahpy of the vapor. Wet steam is much like the steam rising from a pot of boiling water.
