0
How much energy is required to change 86.0g of water at 100 degrees Celsius to 86.0g of steam at 100 degress Celsius Explain answer in kilojoules?
Wiki User
∙ 12y ago
2260 kj/kg X 0.086 kg = 194 kj
The heat of vaporization for water is 2260 kj/kg at 1 atmosphere pressure.
Wiki User
∙ 12y ago
Add your answer:
Earn +20 pts
How much heat is required to convert 1.00 kg of water at 100 degrees Celsius to steam at 100 degrees Celsius?
Assuming standard atmospheric pressure, 2260 kilojoules.
How many kilojoules are required at 0 degrees Celsius to melt an ice cube with a mass of 25g?
To melt 25g of ice at 0 degrees Celsius, you need 334 J/g of energy (latent heat of fusion of ice). To convert this to kilojoules: 334 J/g * 25g = 8350 J = 8.35 kJ.
How much heat in kilojoules must be removed from glass of water that contains 100g of water to lower its temperature from 30 degrees Celsius to 15 degrees Celsius?
6.276 kJ
How much heat in kilojoules must be removed from a glass of water that contains 100g of water to lower it's temperature from 30 degrees Celsius to 15 degrees Celsius?
6.276 kJ
What is the difference between 28 degrees Celsius and 25 degrees Celsius explain?
The main difference between 28 degrees Celsius and 25 degrees Celsius is the temperature value itself. In terms of how it feels, 28 degrees Celsius is typically perceived as warmer than 25 degrees Celsius. This difference may be noticeable in terms of comfort and the need to adjust clothing or activities accordingly.
How many kilojoules of energy are necessary to raise the temperature of 3 kilograms of cast iron from 30 degrees celsius to 120 degrees celsius?
I will use this formula. Some conversion will be required. ( I only know specific heat iron in J/gC ) q(Joules) = mass * specific heat * change in temperature Celsius 3 kilograms cast iron = 3000 grams q = (3000 g)(0.46 J/gC)(120 C - 30 C) = 124200 Joules (1 kilojoule/1000 joules) = 124.2 kilojoules of energy needed ===========================
How much heat energy in kilojoules is required to convert 41.0g of ice at -18.0 degrees C to water at 25.0 degrees C?
The total heat energy required can be broken down into two steps: first, raising the temperature of ice from -18.0°C to 0°C, then melting the ice at 0°C to water at 25.0°C. The heat energy required is calculated using the formula: Q = mcΔT, where Q is heat energy, m is mass, c is specific heat capacity, and ΔT is the temperature change. Step 1: Raise temperature of ice to 0°C Q1 = 41.0g * 2.09 J/g°C * 18.0°C = 1552.22 J Step 2: Melt ice at 0°C Q2 = 41.0g * 334 J/g = 13694 J Total heat energy required = Q1 + Q2 = 13694 J + 1552.22 J = 15246.22 J Convert J to kJ: 15246.22 J * (1 kJ / 1000 J) ≈ 15.25 kJ Therefore, approximately 15.25 kJ of heat energy is required to convert 41.0g of ice at -18.0 degrees C to water at 25.0 degrees C.
How much energy is required to transform solid water at 0 degrees Celsius to liquid at 0 degrees Celsius?
80cal/g
How do you convert 2.35 kilojoules of heat to degree celsius?
To convert 2.35 kilojoules of heat to degrees Celsius, you need to know the specific heat capacity of the substance being heated. Once you have this value, you can use the formula: Heat energy (in joules) = mass * specific heat capacity * change in temperature. By rearranging the formula, you can calculate the change in temperature in degrees Celsius.
The temperature required to boil water at?
100 degrees Celsius
Would a balloon filled with minus 2 degrees Celsius air move to room temperature of 8 degrees Celsius Explain?
A balloon filled with -2 degrees Celsius air will move to a room to a temperature of 8 degrees Celsius because of the collision of the air particles.
How much heat in joules is required to convert 92g of ice at 0.00 degrees Celsius to water vapor at 148 degrees Celsius?
Can you help
