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

Step-by-step solution

According to the first law of thermodynamics, the heat supplied Q is equal to the sum of the change in internal energy U and the work done W by the system during the process of vaporisation. Q = U + W Given that the latent heat of vaporisation L = 2240 J for 1 g of water, the heat supplied Q is 2240 J . The work done W during the process is given as 168 J . Substituting these values into the equation: 2240 J = U + 168 J Solving for the change in internal energy U : U = 2240 J - 168 J U = 2072 J Answer: 2072 J