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If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is re
If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is required to convert 0.5 kg of water at 100°C to steam at 100°C?
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Practice Questions
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Q1
If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is required to convert 0.5 kg of water at 100°C to steam at 100°C?
1130 kJ
2260 kJ
3390 kJ
4520 kJ
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Energy required = mass * latent heat = 0.5 kg * 2260 kJ/kg = 1130 kJ.
Questions & Step-by-step Solutions
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Q
Q: If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is required to convert 0.5 kg of water at 100°C to steam at 100°C?
Solution:
Energy required = mass * latent heat = 0.5 kg * 2260 kJ/kg = 1130 kJ.
Steps: 6
Show Steps
Step 1: Identify the mass of water you want to convert to steam. In this case, it is 0.5 kg.
Step 2: Identify the latent heat of vaporization of water, which is given as 2260 kJ/kg.
Step 3: Use the formula to calculate the energy required: Energy required = mass * latent heat.
Step 4: Substitute the values into the formula: Energy required = 0.5 kg * 2260 kJ/kg.
Step 5: Perform the multiplication: 0.5 * 2260 = 1130 kJ.
Step 6: Conclude that the energy required to convert 0.5 kg of water at 100°C to steam at 100°C is 1130 kJ.
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