Which of the following are not state functions?

(I) q + W                        (II) q

(III) W                           (IV) H-TS

1. (I) and (IV)                     

2. (II), (III) and (IV)

3. (I) , (II) and (III)               

4.  (II) and (III)

Consider the following reactions :

(i) ${\mathrm{H}}^{+}\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>∆\mathrm{H}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-{\mathrm{x}}_1<mspace\; width="1em"></mspace>\mathrm{kJ}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}$

(ii) ${\mathrm{H}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>∆\mathrm{H}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-{\mathrm{x}}_2<mspace\; width="1em"></mspace>\mathrm{kJ}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}$

(iii) ${\mathrm{CO}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>\mathrm{CO}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>∆\mathrm{H}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-{\mathrm{x}}_{3<mspace\; width="1em"></mspace>}\mathrm{kJ}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}$

(iv) ${\mathrm{C}}_2{\mathrm{H}}_5\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\frac{5}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>2{\mathrm{CO}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)<mspace\; width="1em"></mspace>∆\mathrm{H}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-{\mathrm{x}}_4<mspace\; width="1em"></mspace>\mathrm{kJ}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}$

Enthalpy of formation of H₂O(l) is:

1. -x₂ kJ mol^-1 

2. +x₃ kJ mol^-1

3. -x₄ kJ mol^-1

4. -x₁ kJ mol^-1

Identify the correct statement for change of Gibbs energy for a system ($∆$G_system) at constant temperature and pressure:

(1) If $∆$G_system > 0, the process is spontaneous

(2) If $∆$G_system = 0, the system has attained equilibrium

(3) If $∆$G_system = 0, the system is still moving in a particular direction

(4) If $∆$G_system < 0, the process is not spontaneous

The enthalpy and entropy change for the reaction :

Br₂ (l) + Cl₂ (g)$\to$ 2BrCl (g)

are 30 kJ mol^-1 and 105 J K^-1 mol^-1 respectively.

The temperature at which the reaction will be in equilibrium is :

The enthalpy of combustion of H₂, cyclohexene (C₆H₁₀) and cyclohexane (C₆H₁₂) are -241, -3800 and -3920 kJ per mol respectively. Heat of hydrogenation of cyclohexene is:

(a) -121 kJ per mol

(b) +121 kJ per mol

(c) +242 kJ per mol

(d) -242 kJ per mol

Consider the reactionat 300K

H₂₍₉₎ + Cl₂₍₉₎ →2HCI_(g), ΔH° = — 185 KJ

If 3 mole of H₂ completely react with 3 mol of Cl₂ to form Cl, $∆$U° of the reaction will be

(1) Zero

(2) –185 KJ

(3) -555 KJ

(4) None

For a perfectly crystalline solid C_pm = aT³, where a is constant. If C_pm is 0.42 J/K–mol at 10 K, molar entropy at 10 K is

1. 0.42 J/K–mol

2. 0.14 J/K–mol

3. 4.2 J/K–mol

4. zero

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300 K then total entropy change of system in the above process is :

[R = 0.082 L atm mol^–1 K^–1 = 8.3 J mo1^–1K^–1].

(1) 0

(2) Rln (24.6)

(3) Rln (2490)

(4) $\frac{3}{2}$Rln(24.6)

At 1000 K water vapour at 1 atm. has been found to be dissociated into H₂ and O₂ to the extent of 3 x 10^–6 %.Calculate the free energy decrease of the system, assuming ideal behaviour.

(1) –ΔG = 90,060 cal

(2) –ΔG = 20 cal

(3) –ΔG = 480 cal

(4) –ΔG = –45760 cal

An ideal gas is taken from the same initial pressure P₁ to the same final pressure P₂ by three different processes. If it is known that point 1 corresponds to a reversible adiabatic and point 2 corresponds to a single stage adiabatic then

(1) Point 3 may be a two stage adiabatic.

(2) the average K.E. of the gas is maximum at point 1

(3) Work done by surrounding in reaching point number '3' will be maximum

(4) If point4 and point 5 lie along a reversible isotherm then T₅ < T₁.