The latent heat of vaporisation of water is 2240 J . If the work done in the process of vaporisation of 1 g is 168 J , the increase in internal energy is
The latent heat of vaporisation, also known as the enthalpy of vaporisation, reflects the energy required to transform a substance from a liquid phase to a gas phase without changing its temperature. According to the first law of thermodynamics, the change in internal energy (∆U) during the process of vaporisation can be calculated using the formula: ∆U=Q−W Where: Q is the heat added (latent heat of vaporisation) W is the work done in the process In this scenario: The latent heat of vaporisation (Q) is 2240 J . The work done (W) is 168 J . Substituting these values into the equation, we get:
∆U=2240J−168J Therefore, ∆U=2072J Hence, the increase in internal energy is: Option B: 2072 J