The C-Cl bond energy can be calculated from :

1. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) only$

2. ${{∆}^{\circ }}_f\left(CC{l}_4, l\right) and ∆\left(C{l}_2\right)$

3. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) ∆\left(C{l}_2\right)$

4. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) ∆\left(C{l}_2\right), ∆{H^{\circ }}_f\left(C, g\right) and ∆{H^{\circ }}_{vap}\left(CC{l}_4\right)$

Given $∆{H^{\circ }}_f$ of DyCl₃ (s) = -994.30 kJ mol^-1

$\frac{1}{2}{H}_2\left(g\right)+\frac{1}{2}C{l}_2\left(g\right)\stackrel{+aq}{\to }HCl\left(aq. 4 M\right); ∆H^{\circ }=-158.31 kJ mo{l}^{-1}$
$DyC{l}_3\left(s\right)\underset{HCl}{\overset{aq}{\to }}DyC{l}_3\left(aq. 4 M HCl\right); ∆H^{\circ }=-180.06 kJ mo{l}^{-1}$
$Dy\left(s\right)\underset{aq. 4 M}{\overset{+3 HCl}{\to }}DyC{l}_3\left(aq. 4 M HCl\right)+\frac{3}{2}{H}_2\left(g\right); ∆H^{\circ }=x, calculate x.$
$$

1. -966.5 kJ/mol

2. -699.43 kJ/mol

3. -596.6 kJ/mol

4. -569.6 kJ/mol

When 1 g H₂ gas at S.T.P is expanded to twice its initial volume, then the work done is:

1. 22.4 L atm
2. 5.6 L atm
3. 11.2 L atm
4. 44.8 L atm

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

If $∆G=∆H-T∆S$ and $∆G=∆H+T{\left(\frac{d\left(∆G\right)}{dT}\right)}_P$ then variation of EMF of a cell E, with temperature T, is given by

1. $\frac{∆H}{nF}$ 

2. $\frac{∆G}{nF}$

3. $\frac{∆S}{nF}$

4. $-\frac{∆S}{nF}$

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

$C_P-C_V=R$. This R is :

1. Change in K.E.

2. Change in rotational energy

3. work done which system can do on expanding the gas per mol per degree increase in temperature

4. All correct

Heat of neutralisation of oxalic acid is -25.4 K cal mol^-1 using strong base, NaOH. Hence enthalpy change of the process is $H_2{C}_2{O}_4\rightleftharpoons 2H^{+}+C_2{H_4}^{2-}$is-

1. 2.0 kcal

2. -11.8 kcal

3. 1.0 kcal

4. -1.0 kcal

5 moles of nitrogen gas are enclosed in an adiabatic cylindrical vessel. The piston itself is a rigid light cylindrical container containing 3 moles of Helium gas. There is a heater which gives out a power 100 cal to the nitrogen gas. A power of 30 cal is transferred to Helium through the bottom surface of the piston.

The rate of increment of temperature of the nitrogen gas assuming that the piston moves slowly :

1. 2K/sec

2. 4K/sec

3. 6K/sec

4. 8K/sec

During the isothermal mixing of ideal gases at pressure, p, the entropy change per mole for the mixing process is-R $\sum x_i \ln x_i$ where x₁, x₂,....,x_i are the mole fractions of the components, 1, 2,....,i of the mixture. Assuming ideal gas behavior, calculate $∆S$ for the mixing of 0.8 mole of N₂ and 0.2 mole of O₂.(at ${25}^{\circ }C$ and 0.9 atm) [1 eu = cal/deg]

1. 0.9943 eu

2. 0.7533 eu

3. 0.6798 eu

4. 0.7112 eu