Consider the reaction

N₂(g) + 3H₂(g)$\to$2NH₃(g) carried out at constant temperature and pressure. If $∆$H and $∆$E are enthalpy change and internal energy change respectively, which of the following expression is True?

$$\begin{gathered} 1.<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>∆\mathrm{H}⩾∆\mathrm{E}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace> \\ 2.<mspace\; width="1em"></mspace>∆\mathrm{H}=∆\mathrm{E} \\ 3.<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>∆\mathrm{H}<∆\mathrm{E}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace> \\ 4.<mspace\; width="1em"></mspace>∆\mathrm{H}>∆\mathrm{E} \end{gathered}$$

Under which process is the maximum work achieved?

1. Isobaric work           

2. Isothermal work

3. Isochoric work         

4. Adiabatic work

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

Which of the following conditions should be satisfied for the given reaction to be spontaneous at 0$°$C and 1 atm?

H₂O(s) $\rightleftharpoons$H₂O(l)

(1) $∆\mathrm{H}=∆\mathrm{G}$

(2) $∆\mathrm{H}<\mathrm{T}.∆\mathrm{S}$

(3) $∆\mathrm{H}>\mathrm{T}.∆\mathrm{S}$

(4) $∆\mathrm{H}=\mathrm{T}.∆\mathrm{S}$

'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

An ideal gas expands at a constant external pressure of 2.0 atmosphere by 20 litre and absorbs 10kJ of heat from surrounding. What is the change in internal energy of the system:-

(1) 4052 J

(2) 5948 J

(3) 14052 J

(4) 9940 J

36 ml of pure water takes 100 sec to evaporate from a vessel and heater connected to an electric source which delivers 806 watt. The $∆{\mathrm{H}}_{\mathrm{vaporisation}}$ of H₂O is:-

(1) 40.3 kJ/mol

(2) 43.2 kJ/mol

(3) 4.03 kJ/mol

(4) None of these

5 moles of an ideal gas expands isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm. find the W_irr at 300 K:-

1. -15.921 kJ

2. -11.224 kJ

3. -110.83 kJ

4. None of these

In the reaction at 300 K

H₂(g) + Cl₂(g)$\to$2HCl(g)       $∆\mathrm{H}°$= -185 kJ

if 2 mol of H₂ completely react with 2 mole of Cl₂ to form HCl. What is $∆\mathrm{U}°$ for this reaction?

(1) 0

(2) -185 kJ

(3) -370 kJ

(4) None of these

Which of the following reactions has/have a positive \(\Delta S\) (entropy change)?

(i) Ag⁺ (aq) + Cl^-(aq) $\to$AgCl(s)

(ii) NH₄Cl(g) $\to$NH₃(g) + HCl(g)

(iii) 2NH₃(g)$\to$N₂(g) + 3H₂(g)

1. (i) & (ii)

2. (iii)

3. (ii) & (iii)

4. (ii)