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

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

The gas absorbs 100 J heat and is simultaneously compressed by a constant external pressure of 1.50 atm from 8 lit. to 2 lit. in volume. Hence $∆E$ will be-

1. -812 J

2. 812 J

3. 1011 J

4. 911 J

The standard heat of combustion of Al is -837.8 kJ mol^-1 at ${25}^{\circ }C$ which of the following releases 250 kcal of heat ?

1. The reaction of 0.624 mol of Al

2. The formation of 0.624 mol of Al₂O₃

3. The reaction of 0.312 mol of Al

4. The formation of 0.150 mol of Al₂O₃

Following reaction occurs at ${25}^{\circ }C$ :

$$\begin{gathered} 2NO\left(g,<mspace\; width="1em"></mspace>1\times {10}^{-5}<mspace\; width="1em"></mspace>atm\right)+C{l}_2\left(g,<mspace\; width="1em"></mspace>1\times {10}^{-2}<mspace\; width="1em"></mspace>atm\right) \\ \rightleftharpoons 2NOCl\left(g,<mspace\; width="1em"></mspace>1\times {10}^{-2}<mspace\; width="1em"></mspace>atm\right) \\ {∆}^{\circ }G<mspace\; width="1em"></mspace>is<mspace\; width="1em"></mspace>: \end{gathered}$$

1. -45.65 kJ

2. -28.53 kJ

3. -22.82 kJ

4. -57.06 kJ

The bond energies of$C\equiv C$, C-H, H-H and C=C are 198, 98, 103 and145 kcal respectively. The enthalpy change of the reaction $HC\equiv CH+H_2\to C_2{H}_4$ is:

1. 48 kcal

2. 96 kcal

3. -40 kcal

4. -152 kcal

The enthalpies of formation of CO₂(g) and CO(g) at 298 K are in the ratio 2.56 : 1. For the reaction,

$C{O}_2\left(\mathrm{(g)}\right)+C\left(\mathrm{(s)}\right)\to 2CO\left(\mathrm{(g)}\right),<mspace\; width="1em"></mspace>∆H=177.5kJ,$
$∆H_f<mspace\; width="1em"></mspace>of<mspace\; width="1em"></mspace>CO\left(\mathrm{(g)<mspace\; width="1em"></mspace>}\right)i\mathrm{s-}$

1. -150.6 kJ mol^-1

2. -113.78 kJ mol^-1

3. -130.2 kJ mol^-1

4. -141.8 kJ mol^-1

The enthalpies of the following reactions are shown alongwith.

$\frac{1}{2}{H}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\to OH\left(g\right)<mspace\; width="1em"></mspace>;<mspace\; width="1em"></mspace>∆H=42.09<mspace\; width="1em"></mspace>kJ<mspace\; width="1em"></mspace>mo{l}^{-1}$
$H_2\left(g\right)\to 2H\left(g\right);<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>∆H=435.89<mspace\; width="1em"></mspace>kJ<mspace\; width="1em"></mspace>mo{l}^{-1}$
$O_2\left(g\right)\to 2O\left(g\right);<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>∆H=495.05<mspace\; width="1em"></mspace>kJ<mspace\; width="1em"></mspace>mo{l}^{-1}$

Calculate the O-H bond energies for the hydroxyl radical.

1. 223.18 kJ mol^-1

2. 423.38 kJ mol^-1

3. 513.28 kJ mol^-1

4. 113.38 kJ mol^-1

4.8 g of C(diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of formation gaseous carbon is 725 kJ/mol. The energy required for the process

(i) $\mathrm{C}\left(\mathrm{graphite}\right)\to \mathrm{C}\left(\mathrm{gas}\right)$

(ii) $\mathrm{C}\left(\mathrm{diamond}\right)\to \mathrm{C}\left(\mathrm{gas}\right)$are

1. 725, 727

2. 727, 725

3. 725, 723

4. None of these