One mole of a real gas is subjected to heating at constant volume from$\left(P_1, V_1, T_1\right)$ state to $\left(P_2, V_2, T_2\right)$ state. Then it is subjected to irreversible adiabatic compression against constant external pressure of P₃ atm till syatem reaches the final state$\left(P_3, V_3, T_3\right)$. If the constant volume molar heat capacity of real gas is C_V. Find out correct expression for $∆H$ from state 1 to state 3-

1. $C_v\left(T_3-T_1\right)+\left(P_3{V}_1-P_1{V}_1\right)$

2. $C_v\left(T_2-T_1\right)+\left(P_3{V}_2-P_1{V}_1\right)$

3. $C_v\left(T_2-T_1\right)+\left(P_3{V}_1-P_1{V}_1\right)$

4. $C_p\left(T_2-T_1\right)+\left(P_3{V}_1-P_1{V}_1\right)$

The heat evolved in the combustion of 112 litres of water gas(mixture of equal volumes of H₂ and CO) is:

1. 241.8 kJ

2. 283 kJ

3. 1312 kJ

4. 1586 kJ

In which case of mixing of a strong acid and a base, each of 1(N) concentration, temperature-increase is the highest ?

1. 20 ml acid and 30 ml alkali

2. 10 ml acid and 40 ml alkali

3. 25 ml acid and 25 ml alkali

4. 35 ml acid and 15 ml alkali

The heats of neutralisation of four acids A, B, C and D are -13.7, -9.4, -11.2 and -12.4 kcal respectively when they are neutralised by a common base. The acidic character obeys the order :

1. A>B>C>D

2. A>D>C>B

3. D>C>B>A

4. D>B>C>A

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