Why does steam have a lower specific heat than water?
First we must understand that there is a direct correlation between temperature of a substance and the amount of molecular movement. At absolute zero the molecules do not move at all. As the temperature increases, so does movement. As movement increases, so does temperature.
Water has two hydrogen atoms and one oxygen atom. The oxygen of one water molecule has two lone pairs of electrons. Each can form a hydrogen bond with the hydrogen on two other water molecules. This repeats so that every water molecule is bonded to four others (two through its lone pairs and two through its two hydrogen atoms.) These bonds restrict movement.
Since heat makes molecules move and the hydrogen bonds resist this movement, it takes more energy to break the bonds of liquid water and force the molecules apart into a gaseous state. Once transformed to a gas, there are fewer bonds to overcome, so the energy to make the molecules move (heat them up) is lower.
Because steam is actually hotter than water AT FIRST, but after it gets into the atmosphere it lowers which is why it condensates (condenses) on a wall or glass or something. Because it lowers heat, it sticks.
Does it take more energy as heat to raise the temperature of water by one degree than to raise the temperature of steam by the same amount?
How do you calculate the total heat required in kcal to take 70 grams of ice at -29.0 Celsius and convert it to steam at 106 Celsius?
heat energy required to raise the temperature of ice by 29 celsius =specific heat capacity of ice * temperature change *mass of ice + to change 1kg of ice at 0 celsius to water at 0 celsius =specific latent of fusion of ice*mass of water + heat energy required to raise the temperature of water by 106 celsius =specific heat capacity of water * temperature change *mass of ice + to change 1kg of water…
The heat of evaporation of 1 gram of water at 100C at atmospheric pressure is 538.5 calories. 1 gram of water condensing from a 100% quality of saturation (dry steam) at 100C and atmospheric pressure releases 538.5 calories. For lower quality the enthalpy is lower. Such that the latent heat of evaporation is reduced by the amount of moisture in the steam.
Soil does not have a higher specific heat than water. Specific heat capacity, also known simply as specific heat (Symbol: C or c) is the measure of the heat energy required to raise the temperature of one gram of a substance by one Kelvin (or degree Celsius). Water has a specific heat of 1 calorie / gram / degree C. The specific heat of dry is soil is ~ 0.2 calorie / gram / degree…
Alike... Both have a Specific heat value of 0.5 Both are another state of water --------------------------------------------------------- Different... Ice is 32 Deg F and below while steam is 212 Deg. F and above To change water to ice you need 144 BTU (latent heat of fusion) To change water to steam you need 970.3 BTU (latent heat of evaporation)
Heat, as distinct from temperature, can only be measured using a medium, ie a substance of known specific heat. Then by measuring its temperature the amount of heat can be calculated. Water is the easiest to use, at least up to its boiling point, and by definition, a rise of 1 deg C per gram of water is 1 calorie. One of the most frequent needs to measure heat is in power stations or industrial…
Station heat rate = Specific fuel consumption * Calorific value of fuel Turbine heat rate = (Main steam flow * Main steam enthalpy + Aux Steam flow * Aux steam enthalpy - Feed water flow * Feed water enthalpy + Makeup water flow* Makeup water enthalpy)/Power generation Unit of Heat rate is kcal/kWh, kJ/kWh,Mcal/MWh, MJ/MWh, Turbine efficiency = 1/ turbine heat rate for Kcal/KWh is 860/ turbine heat rate For kJ/kWh is 3600/turbine heat rate…
How many joules of energy are needed to heat 25.0 grams of steam from 100.0 degrees Celsius to 29.25 degrees Celsius?
Use this formula. q(in Joules) = Mass * specific heat * change in temperature I will use specific heat of water at 25 C. You can look up specific heat of steam. You say " heat to " so I assume you have final and initial heat backwards. q = 25.0 grams H2O * 4.180 J/gC * (100.0 C - 29.25 C ) q = 7393 Joules
It is because the density increases as you add salt and with all other substances the higher the density the lower the specific heat. For example water has a density of 1000 Kg m -3 and a specific heat of 4186 J/Kg. On the other hand copper has a density of 8960 Kg m -3 and a specific heat of 385 J/Kg.
For example, water and air at 100°C. Water at 100°C takes in more heat to convert to gaseous state, that is, steam. Since steam takes in heat, it is found to be hotter than water. Another example: Hot water does not cause as much damage to skin tissues as steam, since steam has a lot of latent heat energy. Ice takes in a certain amount of heat energy to change to water. Then, water takes…
Actually when steam condenses it is loosing heat. As steam rises it cools and falls back down with gravity. I.E. a steam boiler heat system Boils water to till it turns into a gaseous mixture of water droplets and rises to a radiator to heat. As the radiator absorbs the heat from the steam It condenses and returns to the boiler through the same riser pipe to the boiler.
Water is used to transfer heat from the nuclear fuel in the reactor to the steam generators where it transfers heat to the secondary water to make steam. The steam is then used to turn turbines. Water from an external source is also used to condense the steam from the turbine exhaust, and this water is then returned to the steam generators to continue the cycle.