How much energy is released when 1 gram of steam condenses to water at 100 degrees Celsius?
To determine the amount of energy released when 1 gram of steam condenses to water at 100 degrees Celsius, we need to use the concept of specific heat and latent heat of vaporization.
First, we need to calculate the amount of energy required to heat the water from its initial temperature (let's assume it is 0 degrees Celsius) to its boiling point of 100 degrees Celsius. The specific heat capacity of water is 4.18 J/g°C, which means it takes 4.18 Joules of energy to heat 1 gram of water by 1 degree Celsius. So, to heat 1 gram of water from 0 to 100 degrees Celsius, we would need:
Q1 = mass × specific heat × temperature change
= 1 gram × 4.18 J/g°C × (100°C - 0°C)
= 418 Joules
Next, we need to calculate the energy required for the phase change from steam to liquid water at its boiling point. The latent heat of vaporization for water is approximately 2260 J/g. This means that for 1 gram of steam to condense to water at 100 degrees Celsius, it releases 2260 Joules of energy.
So, the total energy released when 1 gram of steam condenses to water at 100 degrees Celsius is the sum of the energy required for heating and the energy released during condensation:
Total energy released = Q1 + Q2
= 418 Joules + 2260 Joules
= 2678 Joules
Therefore, when 1 gram of steam condenses to water at 100 degrees Celsius, it releases approximately 2678 Joules of energy.