The change of ice to water at 273 K in a thermodynamics reversible maner is represented below. `ice harr water (i)`, DeltaH = 6.61 kJ//mol, reversible
Predict the entropy change of the surrounding from the above answer.

Molar enthalpy change for vapourisation of 1 mol of water at 100^@C and 1 bar pressure is 41 kJ mol^-1 . Assuming water vapour to be a perfect gas, calculate the internal energy change when (ii) 1 mol of water is converted to ice

Enthalpy and Entropy changes of two reactions are given below: Find out whether they are spontaneous or not at 27^oC . Justify. a) DeltaH = 26 kJ/mole, DeltaS = 8.3 J/K/mole b) DeltaH=-393.4 kJ/mole, DeltaS = 6 J/K/mole

Categorise in to reversible and irreversible process. (i) Water fall, (ii) rusting of iron, (iii) electrolysis, (iv) diffusion of gas. (v) melting of ice, (vi) dissolving NaCl in water, (vii) flow of heat from hot body to cool body

a) Predict whether entropy increases or decreases in the following changes: i) l_2(S)rightarrowl_2(g) ii) Temperature of a crystalline solid is raised from 0 K and 115 K. iii) Freezing of water b) Calculate the enthalpy of combustion of methane. Given that standard enthalpies of formation of CH_4,CO_2 and H_2O are -75.2, -394 and -285.6 kJ/mol respectively.

In the following changës, state whether order has increased or decreased and con-, sequently the sdirection of change of entropy of the system? i) Steam 'rarr' water ii) 'H_2 O(l) rarr H_2 O(s)' iii) Normal 'egg rarr' hard boiled egg. iv) Dry ice (solid carbon dioxide) 'rarr CO_2(g)'.

For the melting of ice at '25^circ C' : 'H_2 O(s) rarr H_2 O(l)' the enthalpy of fusion is '6.97 kJmol^(-1)', and entropy of fusion is '25.4 J mol^(-1) K^(-1)'. Calculate the free energy change and predict whether melting of ice is spontaneous or not at this temperature.