The $∆H_f^{\circ }$ for CO₂(g), CO(g) and H₂O(g) are -393.5, -110.5 and -241.8 kJ mol^-1 respectively. The standard enthalpy change (in kJ) for the reaction,

$C{O}_2\left(g\right)+H_2\left(g\right)\to H_{2}O\left(g\right)+ CO\left(g\right)$ is :

1. 524.21

2. 41.2

3. -262.5

4. -41.2

The dissociation energy of CH₄ and C₂H₆ are respectively 360 and 620 Kcal/mole. The bond energy of C-C is-

1. 260 Kcal/mole

2. 180 Kcal/mole

3. 130 Kcal/mole

4. 80 Kcal/mole

For an endothermic reaction-

1. $\sum _{Products}H=\sum _{Reac\tan ts}H$

2. $\sum _{Products}H<\sum _{Reac\tan ts}H$

3. $\sum _{Products}H>\sum _{Reac\tan ts}H$

4. $\sum _{Products}H=0 but \sum _{Reac\tan ts}H is positive.$

All the natural process in this universe produce

1. A decrease in entropy of the universe

2. An increase in entropy of the universe

3. No change in entropy

4. Sometimes increase or sometimes decrease in entropy

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