The correct calculate value for $△H$ for:

$\mathrm{M}\left(\mathrm{s}\right) \to {\mathrm{M}}^{2+}\left(\mathrm{aq}\right)$

From following arbitrary values : 

$\mathrm{M}\left(\mathrm{s}\right) \to \mathrm{M}\left(\mathrm{g}\right) ;△\mathrm{H} = 1000\mathrm{KJ} {\mathrm{mol}}^{-1}$
$\mathrm{M}\left(\mathrm{g}\right) \to {\mathrm{M}}^{+}\left(\mathrm{g}\right) ; △\mathrm{H} = 750\mathrm{KJ} {\mathrm{mol}}^{-1}$
${\mathrm{M}}^{+}\left(\mathrm{g}\right)\to {\mathrm{M}}^{2+}\left(\mathrm{g}\right);△\mathrm{H} = 1200\mathrm{KJ} {\mathrm{mol}}^{-1}$
${\mathrm{M}}^{2+}\left(\mathrm{g}\right)+\mathrm{aq} \to {\mathrm{M}}^{2+}(\mathrm{aq}.); △\mathrm{H} = -1800\mathrm{KJ} {\mathrm{mol}}^{-1}$

1. 1950 KJ mol^-1 

2. 1150 KJ mol^-1 

3. 2300 KJ mol^-1 

4. None of the above.

The molar heat capacity, $C_v$ of an ideal gas whose energy is that of translational motion only is

1.  $2.98 J de{g}^{-1}mo{l}^{-1}$

2. $12.47 J de{g}^{-1}mo{l}^{-1}$

3. $6.43 J de{g}^{-1}mo{l}^{-1}$

4. $9.41 J de{g}^{-1}mo{l}^{-1}$

The enthalpy of hydration of Na⁺(g) and Cl^-(g) ions are -406 kJ mol^-1 and -364 kJ mol^-1 respectively.
The enthalpy of the solution of NaCl(s) is:
\(\text{The lattice energy of NaCl is}~ 780~{ kJ mol}^{-1}. \)

1. 23 kJ mol^-1

2. 10 kJ mol^-1

3. -10 kJ mol^-1

4. -82 kJ mol^-1

Enthalpy of fusion of a liquid is 1.435 kcal mol^-1 and molar entropy change is 5.26 cal mol^-1K^-1. Hence melting point of liquid is :

1. ${100}^{\circ }C$

2. $0^{\circ }C$

3. 373 K

4. $-{273}^{\circ }C$

ΔG° of the following reaction at 25°C is:

\(2 N O\left(\mathrm{~g} \right)~~~~~+~~~~~~~C l_2\left(\mathrm{~g}\right) ~~~~~~\rightleftharpoons~~~~~~~~~~~ 2 N O C l\left(\mathrm{~g}\right)\\1 \times 10^{-5} \mathrm{~atm}~~~~~~~~1 \times 10^{-2} \mathrm{~atm}~~~~~~~~~~~~~1 \times 10^{-2} \mathrm{~atm}\)

When 1 mole of an ideal gas to 20 atm pressure and 15 L volume expands such that the final pressure becomes 10 atm and the final volume become 60 L. Calculate entropy change for the reaction (C_p.m = 30.96)

1. $80.2 J k^{-1}mo{l}^{-1}$

2. $62.42 J k^{-1}mo{l}^{-1}$

3. $120\times {10}^2 J k^{-1}mo{l}^{-1}$

4. $27.22 J k^{-1}mo{l}^{-1}$

If a process is both endothermic and spontaneous, then :

1. $∆S>0$

2. $∆S<0$

3. $∆H<0$

4. $∆G>0$

The bond energies of C=C and C-C at 298 K are 590 and 331 kJ mol^-1 respectively. The enthalpy of polymerization per mole of ethylene is

1. -70 kJ

2. -72 kJ

3. 72 kJ

4. -68 kJ

1 mole of NH₃ gas at ${27}^{\circ }C$ is expanded adaibatic condition to make volume 8 times ($\gamma$=1.33). Final temperature and work done respectively are-

1. 150 K, 900 cal

2. 150 K, 400 cal

3. 250 K, 1000 cal

4. 200 K, 800 cal

Which of the following statements is correct with regard to $∆$G of a cell reaction and EMF of the cell (E) in which the reaction occurs ?

(1) Both $∆$G and E are extensive properties

(2) $∆$G is an intensive property but E is an extensive property

(3) $∆$G is an extensive property and E is an intensive property

(4) Both $∆$G and E are intensive properties.