Which of the two contains more heat energy : $1 kg$ of water at $100 ° C$ or $1 kg$ of steam at $100 ° C$ ?

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Solution

Latent heat of vaporisation can be defined as the amount of heat energy that is required to change $1 kg$ of water into its vapour at atmospheric pressure without any change in temperature at its boiling point.
Steam is the gas formed when water passes from the liquid state to the gaseous state.
1 kg of steam contains more heat than 1 kg of water because to convert water into steam, the heat used is more than the actual boiling point. This extra heat is latent heat.
The latent heat of vaporisation for steam at $100 ° C$ is $2.25 \times 10^{6} Joules / kg$ .
Thus, water contains its own heat but steam contains its own heat as well as the latent heat.
Hence, $1 kg$ of steam at $100 ° C$ contains more heat than $1 kg$ of water at $100 ° C$ .

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