The entropy change in the fusion of one mole of a solid melting at 27$°$C  is  -       

(the latent heat of fusion is 2930 J mol^-1)                                                                                   

1. 9.77 JK^-1mol^-1               

2. 19.73 JK^-1mol^-1               

3. 2930 JK^-1mol^-1               

4. 108.5 JK^-1mol^-1          

1 mole of an ideal gas at 25$°\mathrm{C}$ is subjected to expand reversibly ten times of its initial volume. The change in entropy of expansion is:

1. 19.15 JK^-1mol^-1                         

2. 16.15 JK^-1mol^-1

3. 22.15 JK^-1mol^-1                         

4. None of the above

In the reaction, $∆$H and $∆$S both are positive. The condition under which the reaction would not be spontaneous is -

1. $∆$H>T$∆$S                             

2. $∆$S=$∆$H/T

3. $∆$H=T$∆$S                               

4. All of the above

Determine the enthalpy change for the specified reaction:

2H₂O₂(l) $\to$ 2H₂O(l) + O₂(g).

(Given the heat of formation of H₂O₂(l) and H₂O(l) are –188 and –286 kJ/mol respectively)       

Entropy decreases in which of the following reactions?

1. Boiling of egg

2. Combustion of benzene at 127$°$C

3. Stretching of rubber band

4. Dissolution of sugar in water

Equilibrium is represented by:

1. $∆$H = 0             

2. $∆$G_Total=0

3. $∆$S_Total=0         

4. $∆$E=0

Work done is maximum in -

1. Isobaric work           

2. Isothermal work

3. Isochoric work         

4. Adiabatic work

For exothermic reaction to be spontaneous ($∆\mathrm{S}$=negative) temperature must be -

'The free energy change due to a reaction is zero when-

1. The reactants are initially mixed.

2.  A catalyst is added

3. The system is at equilibrium

4. The reactants are completely consumed

For a given reaction, $∆$H =35.5 kJ mol^-1 and $∆$S = 83.6JK^-1 mol^-1. The reaction is spontaneous at:
(Assume that $∆$H and $∆$S do not vary with temperature)