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If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is re

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Question: 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?

Options:

  1. 1130 kJ
  2. 2260 kJ
  3. 3390 kJ
  4. 4520 kJ

Correct Answer: 1130 kJ

Solution: 

Energy required = mass * latent heat = 0.5 kg * 2260 kJ/kg = 1130 kJ.

If the latent heat of vaporization of water is 2260 kJ/kg, how much energy is re

Practice Questions

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?
  1. 1130 kJ
  2. 2260 kJ
  3. 3390 kJ
  4. 4520 kJ

Questions & Step-by-Step Solutions

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?
  • 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.
  • Latent Heat of Vaporization – The amount of energy required to convert a unit mass of a substance from liquid to vapor without a change in temperature.
  • Mass-Energy Relationship – Understanding how to calculate energy based on mass and specific latent heat values.
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