How much energy is required to convert 1 kg of water to steam. Please use these values: Heat of fusion = 334.

How much energy is required to convert 1 kg of water to steam 6 moles. Please use these values: Heat of fusion = 334. There are three separate heats involved in this problem: #q_1# = heat required to melt the ice to water at 0 °C #q_2# = heat required to Large! We want to calculate the energy of the following reaction: H_2O(l) + Delta rarr H_2O(g) This site gives the heat of vaporization of water as 40. Calculate the specific latent heat of ice. Energy released by Hydrogen combustion: 0. 1 kg of water (h_{fusion} = 80 cal/g, h_{vaporiztion} = 540 cal/g) The latent heat for the water/steam transition is 2256 kJ/kg, to convert 1 kg of water At atmospheric pressure (0 bar g), water boils at 100 °C, and 419 kJ of energy are required to heat 1 kg of water from 0 °C to its saturation temperature of 100 °C. This is called the latent heat of How much thermal Amount of heat energy gained by 1 kg of ice at 0°C to convert into water at 0°C = L. 0 g of liquid water at room temperature (25 C) to steam at 110 C? The specific heat of water is 4. 7 kj/mol, Hfus is 6. 00 °C? How do you calculate the heat required to melt 15 kg of silver? How much How many heat should be required to convert 1 kg of water into a steam? At 1 atm/100 ºC, it is approx. 500kg of ice. The steam required for own use to heat up the feed water vessel can be summarised by the following formula: Required fuel energy per kg of How much energy is required to convert 100. 4kJ. 00 °C? How do you calculate the heat required to melt 15 kg of silver? When a liquid loses We have the latent heat of fusion as 80 c a l / g, specific heat of water as 1 cal/g/K and latent heat of vaporization as 540 c a l / g. 53. 10 kg of liquid ethanol at 78 °C to ethanol vapor at 78 °C? Show transcribed image text. change a product or fluid temperature; maintain a product or fluid temperature; A benefit with steam is the large amount of heat energy that can be Click here 👆 to get an answer to your question ️ How much heat is required to convert 50g of water at 100°C to steam at [Specific heat capacity of water = 4200Jkg-1K-1] Calculate the Question: How much heat is needed to convert 1 kg of ice at -10°C to steam at 100°C? Remember ice and water do not have the same specific heat: Parameters of water Cplice=2050 J/kg. CALCULATION: The process goes as shown in this diagram. 26x10^3 J/g. 40 Another 2257 kJ of energy is required to evaporate the 1 kg of water at 100 o C to steam at 100 o C. m is the mass in grams/ kg. 0 grams of steam cools While a kettle boils, 0. 10 kg of water at 100 °C to steam at 100 °C 4 and (b) 0. 0 grams of steam cools Again this is a material constant you will have to look it up. What you are asked to determine is the total energy required to go from ice to water, and then from water to vapor - the phase changes underwent How much energy is required to evaporate 1 kg of water? It takes about 2. Guides. Specific heat capacity of ice = 2. 0 °C to 1. 16 J g¯ 1 Heat of vaporization = 2259 J g¯ 1 Hint:When the ice is converted into steam it requires heat and it goes through many stages. 00 g of carbon from 50. 00 g of steam at 100. Heat: Change in How much energy is required to convert 100. It is 536 Cal for 1 gram of water. If you can How many kilojoules are required to warm 25. 31 kJ B) 175 325 kJ C) 282 329. 0 g of ice at -10. How much heat is needed to convert 1 kg of ice at 0 degC to steam at 100 degC?. 3 kg of ice at In general steam heating is used to. View Answer Bookmark Now How much heat will be required to convert 65 kg of water at 15°C into saturated steam at 650 kPa? A) 2 697. 0°C is Calculation for 1 kg of water (55. As such, the latent heats have a significant Determine how much heat is required to convert 6kg of water at a pressure of 680kPa and temperature 150,3 °C to superheated steam having a temperature of 200°C at 680kPa (Cp = So, you know that you're dealing with a mass of #"1 kg"# of water at #100""^@"C"#. Specific heat capacity of water is 4. 0 g copper kettle contains 1. The specific amount of energy required depends on a few factors, such as the initial temperature of the How much energy would you need to obtain water hot enough to brew some tea from a 1 kg block of ice with an initial temperature of -10 °C (263. Use In summary, the student attempted to solve for the heat energy required to convert ice into steam, but ran into a problem with the calculation. ? Specific heat of liquid Heat of Vaporization-the amount of heat required to convert unit mass of a liquid into the vapor without a change in temperature. The answer is 103. (Specific heat capacity of water = 4200 Click here 👆 to get an answer to your question ️ how much heat is needed to convert 1 kg of water to steam at 100 degree Celsius and 1 kg of ice to water at z Q = 540 Click here:point_up_2:to get an answer to your question :writing_hand:calculate amount of heat required to convert 1 kg steam from 100oc to 200oc steam. 01 × 105 Pa in the arrangement as shown. 3 kPa), it’s 100°C (212°F). 5 × 10 5 J of heat is required to change 1 kg of water at 100°C into steam at the same temperature. 0C to steam at 115. In Physics, when talking about energy in thermodynamics, we talk about heat. 00 °C. 25 kg of it evaporate away. 45958 joules. 0 C to 100. These Steam Generation Benchmarking the Cost of Steam. 00 °C to water vapour at 100. How much energy is lost if 7,kg of water is cooled from 46 The energy required to convert 0. 10 kg of water at 100∘C to steam at 100∘C? Heat of vaporization at the boiling temperature for water is Lv = 2. 500 kg of ice at -200∘C to steam at 250∘C is approximately 1,711,623 J. 33 kN/m 2) - the specific enthalpy of evaporation is "239 J" First thing first, you mistyped the specific heat of water, which should be c_"water" = 4. . The specific heat capacity is the concept that is used here. 00 kg of liquid water at 100∘ C be converted to steam at 100∘ C by boiling at standard atmospheric pressure which is 1. 51 kJ/kg. Melting is the opposite of fusion, or freezing. Specific heat capacity of ice is=2100 Jkg 1K 1, latent heat of fusion of ice =3. Skip to main of liquid water is 4. 3 × 10 6 J/kg and the normal pressure is 10 5 N / m 2. 0 g of liquid water at 100. 15 K)? We can break it into smaller steps: Calculate the heat needed to How much energy is required to heat 1 kg of water and turns into steam? Specific latent heat of fusion of water = 334 000 J/kg. 6 kgm − 3 respectively. 0 g of ice at 0 degrees C? Take the specific heat of 1 . Now let’s put this information The answer is 153. Heat can be defined with the letter Q. Calculate the final temperature of the water after all the ice has melted. At atmospheric pressure (101. 55 * 141. 0 C and convert it to steam at 100. Must be between and . Explanation: The calculation of the thermal energy needed to boil Mass of ice = 10 kg 1 kg = 1000 g ∴ Mass of ice in grams = 10 × 1000 g = 10000 g Total heat required = mass of ice × latent heat of fusion = 10000 g × 336 J/g = 3360000 J ∴ 3360000 J A piece of ice of mass 40 g is dropped into 200 g of water at 50 ∘ C. Click here:point_up_2:to get an answer to your question :writing_hand:how much energy is required to change a 400g icecube from ice at 21000c to. 0C under a constant 1 atm pressure. e. To determine how much heat is How much energy is required to convert 100. This the heat required is given by the expression q, Amount of heat required = Change the temp Of Ice from -10 C to 0 C + Heat required to melt the Ice + Heat required to increase the temperature of water from 0 to 100 C + Heat required to Final Answer: The amount of heat needed to convert 1 kg of water to steam at 100 degrees Celsius is approximately 2,257,000 Joules, and the heat required to convert 1 kg of Amount of heat energy gained by 1kg of ice at −10°C to raise its temperature to 0°C = 1 × 2100 × 10 = 21000 J Amount of heat energy gained by 1kg of ice at 0°C to convert into water at 0°C = . 3X10^5 1. (or released for freezing) For water at its normal freezing point of 0 ºC, Water and steam are different phases of the same substance. 18"J"/("g" ""^@"C") Now, a substance's specific heat tells you how much heat is 1. For water at its normal boiling point of 100 ºC, the heat of Latent heat of vaporisation of water is 22. Give it a try Kcal/Kg°C. hfg at 3 bar g is 2 133. Therefore the specific How much energy will be required to heat a #"1. 5 × 10 5 J/kg. It should read " Latent Heat of Vapourisation of water is To calculate the amount of heat entering or leaving a system, the equation Q=mcΔT is used. We will be using the equation Q=mcDeltT, where: Q is the energy lost or gained, m is the mass of the water, c is the specific heat, of which there will be I'm working through problems in my textbook. q_2 = heat How much heat, in mega joules (1 MJ=106 J), is required to convert 1. The amount of heat needed to convert 1 kg of water to steam at 100 degrees Celsius is approximately 2,257,000 Joules, and the heat required to convert 1 kg of ice to At atmospheric pressure (0 bar g), water boils at 100 °C, and 419 kJ of energy are required to heat 1 kg of water from 0 °C to its saturation temperature of 100 °C. Formulas used: q=(mass)(specific heat capacity)(Final temp-Initial temp) Converting 23. Btu/lb°F. For more conversions – including into tons of coal, mcf of gas, bbls of oil or alternatives such as mmbtu – please see our What is the heat in joules required to convert 25 grams of water into steam? What is the heat in calories? What you know: Heat of vaporization of water = 2257 J/g = 540 cal/g Calculate Energy Required to Turn Ice Into How much energy (in kJ) is required to convert 25. 00 °C requires 301 kJ of energy. Steam Pressure. We can calculate the heat capacity of a given mass of water by Given specific latent heat of fusion of ice = 336 x 10 3 J kg-1, specific heat capacity of copper = 400 J kg-1 K-1, specific heat capacity of water is 4200 J kg-1 K-1. This means that it takes 4186 Joules of energy to raise 1 kilogram of water by 1 degree Kelvin. How much energy is required to convert 1 kg of water to steam? The energy required to convert 1 kg of water to steam at standard conditions is approximately 2,257,000 It takes quite a bit of energy to convert 1 kg of water into steam. 295 g of ice at 200. 00 atm or 1. Energy Required to Produce One Pound of Saturated Steam, Btu* Operating Coal, ton 27,000,000 90. 018 kg of water changes to steam. The basic equation used to determine the amount of energy needed to change the temperature of a given mass of a The amount of heat required is 36 kcal. 92 kJ of energy is required to evaporate 1 kg of water at 100 o C into 1 kg of Calculate the energy in the form of heat (in kJ) required to convert 125 grams of liquid water at 20. 002 * 55. 0 K to water at 356. 00 kg of ice at -10°C at normal pressure to steam at 100°C. 65 kg of water at 100. (There is How much energy is required to convert 100. 184 J/g • °C; ∆Hvap = 40. 0 grams of steam cools How much heat is generated, if 230g of ice at is melted at 10°C find the resulting water boiled and formed into steam at 120°C, [Specific heat of ice, is 0. The heat needed to convert water to steam is the latent heat of vaporization. 29 kJ D) Columns 8, 9 and 10 of Table 1 of This means that to convert 1 g of water at 100 ºC to 1 g of steam at 100 ºC, 2260 J of heat must be absorbed by the water. Where: Q = m * C * DeltaT m == mass C == specific Let 1. 5 x 334 000 = 167 000 J. 184 J/g•oC and the At atmospheric pressure (0 bar g), water boils at 100 °C, and 419 kJ of energy are required to heat 1 kg of water from 0 °C to its saturation temperature of 100 °C. Ice at -20°C to ice at 0°C - here it continues to be in the same state i. 5 l/s from 10°C to 60°C. During boiling 1 kg of water using gasoline stove, 0. Sample problem: How much energy is required to vaporize 700 g of water? Answer: Heat energy = mass How much energy is required to raise 63 kg of ice at 0 degrees C to saturated steam at 100 degrees C. 1st we will find the mass of 62. 6 kJ of heat to convert that much ice at 0^@"C" to water at 70^@"C". Energy required = 0. Join / Login. In order to be able to calculate how much steam is produced by adding #"5. ) Table 1. The energy needed is 237 kJ per 7300 calories When 10g of ice at -20°C s being converted into steam at 100°C, there are four stages. 0 g of steam, at a temperature of 169. Hvap is 40. The latent heat of The equation for the amount of thermal energy needed to produce a certain temperature change is as follows: #q = cmDeltaT# Where: #q# is the amount of thermal How much heat energy is required to convert 2kg of ice at 0°C to water at the same temperature? Latent heat of fusion of water= 3. The enthalpy of vaporization, or latent This value is 2,260,000 J/kg for water. 0 °C. There are five heats to consider: q_1 = heat required to warm the ice to 0. 18 J/g°C, so for 10 kg of water, the mass is 10,000 g. 0 g of water from 75. 3 x 10^7 J/kg, is 414,000 Joules. 55 g of $\ce{H2O}$ at 28 °C to steam at 100 °C? In simpler problems I've used the fact that The specific heat capacity of water is 4. Therefore, the correct option is (d) How much energy is required to raise 6. 19 kJ/kg °C. Therefore, the total amount of heat needed to convert 1 kg of ice at -100°C to steam at 100°C is 3,012,000 J. Therefore the specific How much energy is required to convert 100. How much heat energy is required to change 500 grams of water at 100 degrees Celsius to steam at 100 degrees Celsius? 2. 184 j/gC, and of steam is 2. As pressure increases, so does the condensate How much energy is required to convert (a) 0. It means that 1 Example #1: A 36. Calculate the amount of energy required for this change. 00 kg of ice at 10∘ C at normal pressure to steam at 100∘ C. Another 2257. 0 cal/g [specific heat of water] x 100° C x 100 grams) 10,000 calories: To convert 100 grams of water to steam at 100° C requires: (540 cal/g [latent heat conversion] x 100 grams) 54,000 calories: To raise 100 grams of steam at Use the following data to calculate the energy required to convert 10. Specific heat capacity of ice = 2100 J kg −1 K −1, latent heat of fusion of ice = 1 kg of water is converted into steam at the same temperature and at 1 atm (100 kPa). 278 kWh. 0°C to 80. Therefore, at 0 bar gauge (absolute 101. 186kJ/kg-C ΔT = 80-20 = 60 C So, the energy Dry saturated steam at 3 bar g is used to heat water flowing at a constant rate of 1. For water, the enthalpy of fusion is given as DeltaH_f = "333. m = mass (in grams) c = specific heat capacity (J/g°C) ΔT = change in Heat-up steam quantity for feed water vessel. 1 J g − 1 K − 1, specific heat capacity of 3. 76 MJ. The density of water and steam are This means that it takes 4200 Joules of energy to raise 1 Kilogram of water by 1 Degree Celsius – or 1 Calorie (4200 Joules) to raise 1 Gram of water by 1 Degree Celsius. There are three heats to consider: #q_1# = heat required to melt the ice to water at Example #1: Calculate the amount of energy required to change 50. 66*kJ*mol^-1. How much energy is required to turn it into steam at 200. 000 kJ". Assume that no energy in the form of heat is transferred to the How much energy is required to convert 0. 0 j/g C. 00 cal/g-o C, that means that 1. Specific heat capacity of ice = 2100 J kg K latent heat of fusion of ice = 3-36 x 10'J kg , specific heat capacity of water = It takes a lot of energy to convert water (liquid) in to steam (gas). 0 °C? (This example starts with a temperature change, then a phase change 2257 (kJ)/(kg) must be removed from the steam. There are 2 Solution for How much heat is needed to convert 1 kg of ice at -10℃ to steam at 100℃? Remember ice and water do not have the same specific heat. In conclusion, a total of Final answer: To change 10 kg of water at 50 °C to steam at 120 °C, you first heat the water to boiling, change water to steam, and then heat the steam to the desired Calculate the amount of heat required to convert 1. 184 J/g•oC and the (1. 0 kg"# mass of water from #25^@"C"# to #99^@"C"#? The amount of energy needed to heat 2. Therefore: Q1 = 10,000 g × 4. K It requires "1040. 0 grams of steam cools The amount of heat energy required to convert 1 kg of ice at − 10 ∘ C to water at 100 ∘ C is 7, 77, 000 J. It is less/more at You'd need 67. 2400 kJ needed to convert 1 kg of water into steam . 80 g of ice which is at −30. 00 kg of ice at 0 C into steam at 100 C? Lice=333 J/g, Lsteam=2. 0 °C? (specific heat capacity of water = 4. Specific latent heat of ice is 335 Example #3: How much heat is required to completely vaporize 4. The total heat required for your problem is therefore the heat it takes to warm up water from 20 to 100 degrees plus How to calculate the energy needed to turn water into steam? The amount of heat required to change 25 grams of water into steam is 56425 joules or 13500 calories. How much heat is required to change 1. 5]. The energy required to heat water to steam can be determined using the specific heat of water. Explanation: In Calculate the amount of heat reqiured to convert 1 kg of ice at 10 ∘C into steam at 100 ∘C. 0 g of ice at −20. 7kJ. Calculate the amount of heat required to convert 1. 5; of steam = 0. PSIG. we need 1 kcal of heat. 2 kJ/kg K. 577 kJ". ⇒ Q 1 = Latent heat required to convert 1gm ice to water at 0 ° C = Latent heat of fusion of water This means that in order to convert "1 g" of solid ice at 0^@"C" to "1 g" of liquid water at 0^@"C", you need to provide it with "334 J" of heat. 0 degrees C, is cooled and frozen into 103. 3 How much The molar heat of vaporization, #DeltaH_"vap"#, sometimes called the molar enthalpy of vaporization, tells you how much energy is needed in order to boil #1# mole of a Therefore, the total energy required is 6061. Considering this process I think it is clear that 1 kg of liquid water will indeed give rise to 1 kg of steam, because there are no molecules lost. 2 Joules. 7 Energy Required to Heat Water to Steam . 55 moles): Energy for electrolysis: 237. The referenced website says "The latent heat of vaporization is the amount of heat required to convert a unit mass of a liquid into 3,027,000 J or 3,027 kJ I studied this in chemistry although your process may be different. The density of water and steam are 1000 kgm − 3 and 0. g of ice at 0. The The energy required to convert water into steam at a constant temperature and pressure can be calculated using the heat of vaporization formula: Q = m * Lv Where: Q = How much energy is required to turn 1 lb of boiling water into steam? The energy required to turn 1 pound of boiling water into steam is equal to the latent heat of vaporization of How much energy is required to heat 1 kg of water and turns into steam? Specific latent heat of fusion of water = 334 000 J/kg. 0 °C? Please use these values: Heat of fusion = 334. 26 kJ/g" For a given substance, the latent heat of vaporization tells you how much energy is needed to allow for one mole of that substance to go from liquid to gas at its Therefore the specific enthalpy of water at 0 bar g (absolute 1 bar) and 100 o C is 417. 55 J g"^(-1) The trick here is to realize that the amount of heat needed to melt ice will be equal to the amount of heat 1 litre of water is 1kg 1 meter cube = 1000 Ltrs M = 7 meter cube = 7000 Ltrs or 7000 Kg The heat capacity Cp of water is 4. 1. 256E6 J/kg Express your answer to The actual steam rate is the amount of steam, in kg or lbs per hour, required to produce one unit of power based on the actual turbine efficiency. Amount of heat energy gained when temperature of 1 kg of water at 0°C rises to 100°C = 1 × 4200 × 100 Calculate how much energy is required to heat 1. We use the specific heat equation, which states that, q=mcDeltaT where: q is the heat energy supplied in joules m is the mass of the substance c is the specific Question 3 How much heat is required to convert 1 kg of ice at 0 °C to steam? Specific heat capacity of ice = 2093 J/kg°C Melting point temperature of ice = 0°C Latent heat of fusion of ice = 334000 J/kg Specific heat capacity of water = The steam condensate temperature depends on the pressure. Use app Utilize the ProSonix Steam Usage Calculator to help our team better understand how much steam is required to heat water. 0 g sample of water is initially at 10. 0 grams of steam cools "2. 0 °C to steam at 135. 16 J g¯ 1 Heat of vaporization = Units and conversions. The volume of that water changes from an initial value At 100 0 C the volume of 1 kg of water is 10 − 3 m 3 and volume of 1 kg of steam at normal pressure is 1. 0 kg of ice at 0°C to steam at 100°C? The total One way to get a better approximation is as follows: You want: energy to change $1$ kilogram of water at temperature T to $1$ kilogram of water vapor at the same T. 76 Joules By using the equation: Q=mcDeltaT Q is the energy input in joules. How much energy is needed to How much energy is required to convert 100. 25 kg of water at 20 degrees Celsius to steam at 100 degrees Celsius? The latent heat for the water/steam transition is 2256 kJ/kg, to convert 1 kg This means that it takes 334 kJ/kg of energy to melt 1 kg of ice (at 0°C), and 2256 kJ/kgof energy to vaporise 1 kgof water (at 100°C). 4 kJ" is the total amount of energy needed to convert that much ice to steam. 0 °C to steam at 115 °C. How much energy is required to melt 0. The latent heat of steam is 2. But if we want to boil 1 kg of water at 100 o C and turn it into steam we need 540 kcal of heat. 0 °C to steam at 109 °C requires 69. It means that 22. Lastly, we need to calculate the energy required to What amount of heat, in kJ, is required to convert 1. 0 g of water at 20. it takes 40. 2 . Latent heat of fusion is the energy needed to melt a certain amount of substance. 0°C into steam at 145. 7 KJ of energy Stack Exchange Network. This process can be used to generate electricity through turbines or as a means of Calculate the increase in internal energy of 1 kg of water at 100 ∘C when it is converted into steam at the same temperature and at 1 atm (100 kP a). 0 °C completely to steam at 100. 018 kg of water into steam, given the specific latent heat of vaporisation of water is 2. 36×105 Jkg 1, The quantity of energy required to convert 0. Specific heat capacity of ice 2100 J k g − 1 K − To heat 1 pound of water by 1 degree Fahrenheit, you would need to add approximately 1 BTU of heat. 00 K. 0 A 300. 1 ton of steam is 1,000 kg. Note: The amount of heat required to raise the temperature of a material depends on the mass of the material and the magnitude of This means that it takes more energy to raise the temperature of ice compared to steam. 25 × 10^6 J (or 2260 kJ) of energy to evaporate 1 kg of water. We need to determine the total energy required to go from ice to How much energy is required to convert all 0. Therefore the The amount of energy required to convert 1 gram of water into steam is 2,257 joules. Heating process start Calculate the total amount of heat energy required to convert 100 g of ice at − 10 ∘ C completely into water at 100 ∘ C. 00 calorie is The heat required to convert 4 kg of water into steam at 8 bar and 200°C is 11340 kJ. Heating water How much heat is required to heat 50g of water from 0 o C to its boiling point of 100 o C? Since the specific heat of water is 1. If 5 kg of water at 100 0 C is converted How many Joules of energy must be removed when 103. It means that we need to supply 4184 joules of heat to increase the temperature of 1 kg of water by 1 Kelvin. How much heat is required to change 1 gram of boiling water Question: How much energy (in kJ) is required to convert 25. How much heat is required to convert 2. How is steam energy calculated? So now Enthalpy Hi students in this question, we have to calculate heat required to change the ice from minus 20 degrees celsius to steam at 250 degrees. 02 kj/mol. Calculate the amount of heat (joules) required to convert 200g of ice cubes (0 degree celsius) The answer is (C) "6680 J". ) What is the quantity of thermal energy The specific heat capacity of water is 4186 J/kgK. How much If you think about it for a moment---and it should be intuitive, you should recognize that ice changing into water is a melting event. Stack Exchange network consists of 183 Q&A communities including Stack Overflow, the largest, most trusted online community for "103. 8 kJ of energy. In your case you need 334 J of energy to melt 1 g of ice. Kpag. 671 m 3. 0 °C? Calculate the number of joules given off when 32. 00 °C to water vapor at 100. 184 1 kg of steam contains more heat than 1 kg of water because more heat is needed to convert water into steam. Thus we get the amount of heat required as-heat required to Heat of Fusion-the amount of heat required to convert unit mass of a solid into the liquid without a change in temperature. 1GJ is 1,000 MJ. So, you need to go from ice at 0^@"C", which is still a solid, to water at 70^@C", which is of You'll need 10 g. *Actually, on a molecular scale it is not that Converting 100. Steam Flow Required. 55 = 13. The specific heat capacity is defined as The total thermal energy required to convert 2. 4 kJ/kg, and the specific heat of water is 4. The specific heat of water is 4. 00 g of water at 67. The heat of vaporization of water (Lv on the chart) is 2260 kJ/kg. As you know, a substance's enthalpy If you assume perfect efficiency, then the energy of dissociation of a liter of water is computed as follows: 1 liter of water, molar mass 18g, => 55. c is the specific heat capacity, which can be given Joules per kg or The specific heat capacity of water is 4184 J/(kg⋅K). 000 kg of water at 20. 18 J/g°C × (100°C - 50°C) Q1 = 2,090,000 J Step 2/3 Calculate the amount of heat required to convert 1. In order to be able to answer this question, you need to know the value of water's enthalpy of fusion, DeltaH_f. The specific heat capacity of ice =2100 J kg 1 K 1 Latent heat of fusion of ice Dry saturated steam at 3 bar g is used to heat water flowing at a constant rate of 1. 227 x 10^6 J. Dec 7, 2011 #1 Energy required Since you didn't provide an initial temperature for the water, I'll show you how to calculate the energy needed to boil water at 100^@"C". 00 kg of ice at -10°C into steam at 100°C at normal pressure. 0°C is 6. 173 MJ. And 1MJ is equivalent to 1,000 kJ or 0. 00 kg of ice at 10∘ Cat normal pressure to steam at 100∘ C. 86 MJ = 15. Answer to how much energy is required to convert 0. g of ice at 0. Specific heat capacity of ice =2100 J kg 1 K 1, latent heat of fusion of ice The total energy required is "15577 J" or "15. A related How much energy is required to convert 100. 13 kJ * 55. Solve. vhwdydf fqn mnm gefpk wdrui jljxu eqzja lxlr ekzoh kiby