At `0^(@)C` and 1 atm pressure, the relative amounts of water and ice remain unchanged with time in the equilibrium water `

At 0^(@)C and 1 at pressure, why is the equilibrium established between water and ice regarded as dynamic in nature?

Water and ice remain in equilibrium at 0^(@)C and 1 atm pressure. What will be the value of DeltaG and the sign of DeltaS_("system") at this equilibrium?

The change in enthalpy of vaporisation of 1 mol of water is 40850 " J mol"^(-1) " at " 100^(@)C and 1 atm pressure. What is the difference between molar entropy of water and water vapour at that temperature and pressure ?

At 100^(@)C and 1 atm pressure, the densities of water and water and water vapour are 1.0 g*mL^(-1) and 0.0006 g*mL^(-1) respectively. What is the total volume of water molecules in 1 litre of steam at 100^(@)C ?

Are the following changes reversible or irreversible? Give proper explanations: (i) Melting of ice at 0^(@)C and 1 atm pressure (ii) The pressure of a gas enclosed in a cylinder fitted with a piston is 5 atm. The gas is expanded against an external pressure of 1 atm.

Water remains in equilibrium with its vapour at 100^(@)C and 1 atm. Will the transformation of water into its vapour be spontaneous at this pressure and temperature?

Calculate the values of Delta H and DeltaU in the vaporisation of 90g of water at 100^(@)C and 1 atm pressure. The latent heat of vaporisation of water at the same temperature and pressure =540cal*g^(-1)

What fraction of floating ice remains below the surface of water?

This question has statement I and II. Of the four choices given after the statements, choose the one that best describes the two statements. Statement - I : At ice iff water equilibrium, on increasing the pressure freezing point of water decreases. Statement -II : Ice have low density so equilibrium shift in forward direction when pressure is increased.