Calculate the entropy change in surroundings when 1.00 mole of `H_2O(l)` is formed under standard conditions.
`triangle_fH^@ = 286 kJ mol^-1`.

Calculate the entropy change in the surrounding when 1,00 mol of H_(2)O(l) is formed under standard conditions. Delta_(f)H^(0)=-286kJ*mol^(-1)

Calculate the enthalpy change on freezing of 1.0 mole of water at 10^@C to ice at -10^@C,triangle_(fus)H = 6.03 kJ mol^-1 at 0^@C , C_p[H_2O(l)] = 75.3 J mol^-1 K^-1 C_p[H_2O(s)] = 36.8 J mol^-1 K^-1

Calculate the entropy change involved in the isothermal expansion of 5 mol of ideal gas from a volume of 10 L to 100 L at 300 k

Calculate the entropy change, at 0^@C for the process H_2O(s) rarr H_2O(I) . Given : At 0^@C , H_2O(s) rarr H_2O(g) , Delta H=51885 J. mol^-1 and H_2O(I) rarr H_2O(g) , Delta H=45860 J. mol^-1 .

If the change in entropy of reversible isothermal expansion of 1 mol of an ideal gas is 9.135 " J mol"^(-1). K^(-1) , what will be the entropy change of the surroundings and universe ? If the above expansion of gas is allowed to occur against zero pressure, what will be the entropy change of the system and surroundings ?

Calculate the entropy change at 0^(@) C for the process- H_(2)O(s) to H_(2)O(l) . Given: At 0^(2)C" "C_(2)O(s)toH_(2)O(g),DeltaH=51885J*mol^(-1) and H_(2)O(l)toH_(2)O(g),DeltaH=45860J*mol^(-1) .

Calculate enthalpy change on freezing 1 mol water at 10^(@)C to ice at -10^(@)C. Delta_("fus")H= 6.03 " kJ mol"^(-1) " at " 0^(@)C . C_(p)[H_(2)O(l)]= 75.3 " J. mol"^(-1). K^(-1) , C_(p)[H_(2)O(s)]= 36.8 " J mol"^(-1). K^(-1) .

At 1 atm and 298K DeltaH^(0) value of the reaction 2H_(2)(g)+O_(2)(g)to2H_(2)O(l) is -572 kJ. Calculate the change in entropy of the system and surroundings for this reaction. Is this reaction spontaneous at that temperature and pressure? Given: Standard molar entropies of H_(2)(g),O_(2)(g)&H_(2)O(l) at 298K are 130.6, 205.0 and 69.90 J*K^(-1)*mol^(-1) respectively.

Calculate the free energy change and entropy change per mole when liquid water boils at 1 atmosphere latent heat of vaporization of water= 2.0723KJ mol^(-1)

What is the entropy change for dissolving 1 mole of NaCl at 298 K lattice energy = +777.8KJ mol^(-1) Delta H_(Hydration) of NaCl=-774.1KJ mol^(-1), DeltaG_(dissolution) of NaCl=-914 KJ mol^(-1)