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Water itself does not contain kilojoules (kJ) as it has no caloric value. However, when considering the energy required to heat water, for example, one can calculate the energy in kilojoules based on its mass and the temperature change using the specific heat capacity of water, which is approximately 4.18 kJ/kg°C. Thus, the energy content depends on the context in which the water is being used or heated.
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How many KJ would it take to increase the temperature of 2kg of water by 1c?
To increase the temperature of 2 kg of water by 1°C, you would need 8.4 kJ of energy. This is based on the specific heat capacity of water, which is approximately 4.18 kJ/kg°C. Therefore, for 2 kg, the calculation is 2 kg × 4.18 kJ/kg°C × 1°C = 8.36 kJ, which can be rounded to 8.4 kJ.
How many kJ of energy are required to melt 30.7 g of ice The heat of fusion of water is 6.02 kJmol. The temperature remains constant at 0 and degC. kJ?
10,267 kJ are needed
How many moles of NH4NO3(s) must be dissolved in water so that 73.0 kJ of heat is absorbed from the water?
To determine how many moles of NH4NO3(s) must be dissolved to absorb 73.0 kJ of heat, you need to know the heat of solution (enthalpy change) for NH4NO3. The dissolution of NH4NO3 is typically endothermic, with a heat of solution of about +25.7 kJ/mol. By dividing the total heat absorbed (73.0 kJ) by the heat of solution (25.7 kJ/mol), you find that approximately 2.85 moles of NH4NO3 must be dissolved to absorb that amount of heat.
If the heat of vaporization for water is 2260 Jg how many kilojoules are required to convert 5.00 g of liquid water at 100C to steam at 100C?
The heat required to vaporize 5.00 g of water is given by: 2260 J/g * 5.00 g = 11300 J. Converting this to kJ gives 11.3 kJ.
What volume of water can be boiled by 3.0kJ of energy?
To determine the volume of water that can be boiled by 3.0 kJ of energy, we first need to know the amount of energy required to boil water. The latent heat of vaporization of water is approximately 2260 kJ/kg. Therefore, the volume of water that can be boiled is calculated as follows: [ \text{mass} = \frac{3.0 \text{ kJ}}{2260 \text{ kJ/kg}} \approx 0.00133 \text{ kg} ] Since the density of water is about 1 kg/L, this corresponds to approximately 1.33 mL of water that can be boiled with 3.0 kJ of energy.
How many KJ would it take to increase the temperature of 2kg of water by 1c?
To increase the temperature of 2 kg of water by 1°C, you would need 8.4 kJ of energy. This is based on the specific heat capacity of water, which is approximately 4.18 kJ/kg°C. Therefore, for 2 kg, the calculation is 2 kg × 4.18 kJ/kg°C × 1°C = 8.36 kJ, which can be rounded to 8.4 kJ.
How many kjoules per mole of lithium does the reaction of lithium and water produce?
The reaction of lithium and water produces 286 kJ/mol of lithium.
How many kJ of energy are required to melt 30.7 g of ice The heat of fusion of water is 6.02 kJmol. The temperature remains constant at 0 and degC. kJ?
10,267 kJ are needed
How many kj in 1 apple?
1000 kj, kj means thousand Jules.
How many kj in pizza?
8,000 to 10,000 kJ.
How do I convert the latent heat of condensation of water 334 kJkg into a volumetric measurement of kJ m3?
To convert latent heat of condensation from kJ/kg to kJ/m^3, you need to consider the density of water. The density of water is approximately 1000 kg/m^3. So, multiply the latent heat of condensation (334 kJ/kg) by the density of water (1000 kg/m^3) to get the heat in kJ/m^3, which would be 334,000 kJ/m^3.
How many calories in 350 kj?
350 kJ is 83.6 calories.
How many calories are in 3.97 Kj?
3.97 kJ = 0.95 calories.
How many calories is 8700 kj?
8700 kJ is 2,077.96 calories.
How many calories are in 485 kj?
485 kJ is about 116 calories.
Why does silicon fizz and crack in water?
kj
How many moles of NH4NO3(s) must be dissolved in water so that 73.0 kJ of heat is absorbed from the water?
To determine how many moles of NH4NO3(s) must be dissolved to absorb 73.0 kJ of heat, you need to know the heat of solution (enthalpy change) for NH4NO3. The dissolution of NH4NO3 is typically endothermic, with a heat of solution of about +25.7 kJ/mol. By dividing the total heat absorbed (73.0 kJ) by the heat of solution (25.7 kJ/mol), you find that approximately 2.85 moles of NH4NO3 must be dissolved to absorb that amount of heat.
