For the reaction, $2{\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)$, at 298K $∆\mathrm{H}$ is 164 kJ mol^-1. The $∆\mathrm{E}$ of the reaction is-
1. \(166.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
2. \(141.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
3. \(104.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
4. \(-169 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

For \(A \rightarrow B\), \(\Delta H = 4\ kcal\ mol^{-1}\), \(​​\Delta S = 10\ cal\ mol^{-1}\ K^{-1}\), the reaction is spontaneous when the temperature is:
1. 400 K
2. 300 K
3. 500 K
4. None of the above

44.0 kJ of heat is required to evaporate one mole of water at 298 K. If $∆H_f$ of $H_{2}O\left(l\right)$ is -286 kJ mol^-1, $∆{H^{\circ }}_f$ of $H_{2}O\left(g\right)$ is

1. -330 kJ mol^-1

2. +242 kJ mol^-1

3. -242 kJ mol^-1

4. -198 kJ mol^-1

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. $∆G>0$