The latent heat of vaporisation of water is 2240 J/gm. If the work done in the process of expansion of 1 g of water is 168 J, then increase in internal energy is

The latent heat of vaporisation of water is 2240 J/g . If the work done in the process of expansion of 1 g is 168J then increase in internal energy is

The latent heat of viporisation of water is 2240J if the work done in the process of vaporisation of 1g is 168J the increase in internal energy is

The letent heat of caporisation of water is 2240 J if the work done in the precess of caporization of 1g is 148J then increases in initial energy will be

Latent heat of vaporisation of water is 540 cal/gm.Explain the meaning of the statement.

1g of water changes from liquid to vapour phase at constant pressure of 1 atmosphere, the volume increases from 1 mL to 1671 mL . The heat of vaporisation at this pressure is 540 cal//g . Find the: (a) Work done (in J )during phase change. (b) Increase in internal energy of water.

One gram of water (1 cm^(3)) becomes 1671 cm^(3) of steam at a pressure of 1 atm. The latent heat of vaporization at this pressure is 2256 J/g. Calculate the external work and the increase in internal energy.

1 g of water, of volume 1 cm^3 at 100^@C , is converted into steam at same temperature under normal atmospheric pressure (= 1 xx 10^5 Pa) . The volume of steam formed equals 1671 cm^3 . If the specific latent heat of vaporisation of water is 2256 J/g, the change in internal energy is

A system is provided 50 J of heat and work done on the system is 10 J. The change in internal energy during the process is