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

Which of the following statements is correct with regard to $∆$G of a cell reaction and EMF of the cell (E) in which the reaction occurs ?

(1) Both $∆$G and E are extensive properties

(2) $∆$G is an intensive property but E is an extensive property

(3) $∆$G is an extensive property and E is an intensive property

(4) Both $∆$G and E are intensive properties.

$$\begin{gathered} {\mathrm{C}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)+3.5{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{CO}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) \\ ∆{\mathrm{S}}_{\mathrm{vap}}\left({\mathrm{H}}_2\mathrm{O}, \mathrm{l}\right)={\mathrm{x}}_1 \mathrm{cal} {\mathrm{K}}^{-1}\left(\mathrm{b}.\mathrm{p}. +{\mathrm{T}}_1\right) \\ ∆{\mathrm{H}}_{\mathrm{f}}\left({\mathrm{H}}_2\mathrm{O}, \mathrm{l}\right)={\mathrm{x}}_2; ∆{\mathrm{H}}_{\mathrm{f}}\left({\mathrm{CO}}_2\right)={\mathrm{x}}_3, ∆{\mathrm{H}}_{\mathrm{f}}\left({\mathrm{C}}_2{\mathrm{H}}_6\right)={\mathrm{x}}_4 \\ \mathrm{Hence} ∆\mathrm{H} \mathrm{for} \mathrm{the} \mathrm{reaction} \mathrm{is}- \end{gathered}$$

1. $2x_3+3x_2-x_4$

2. $2x_3+3x_2-x_4+3x_1{T}_1$

3. $2x_3+3x_2-x_4-3x_1{T}_1$

4. $x_1{T}_1+x_2+x_3-x_4$

The molar entropy of the vapourization of acetic acid is\(14.4~ \mathrm{cal}~ \mathrm{K}^{-1} \mathrm{~mol}^{-1}\) at its boiling point ${118}^{\circ }C$. The latent heat of vapourization of acetic acid is-

Which of the following thermodynamic quantities is an outcome of the second law of thermodynamics?

1. Work

2. Enthalpy

3. Internal energy

4. Entropy

From the following data of $∆H$, of the following reactions,

$C\left(s\right)+\frac{1}{2}{O}_2\to CO\left(g\right) ;∆H=-110 kJ$
$C\left(s\right)+H_{2}O\to CO\left(g\right)+H_2\left(g\right) ;∆H=132 kJ$

What is the mole composition of the mixture of steam and oxygen on being passed over coke at 1273 K, keeping temperature constant.

1. 0.5 : 1

2. 0.6 : 1

3. 0.8 : 1

4. 1 : 1

The bond dissociation enthalpy of gaseous H₂, Cl₂ and HCl are 435, 243 and 431 kJ mol^-1, respectively. Calculate the enthalpy of formation of HCl gas.

1. -92 kJ mol^-1

2. -82 kJ mol^-1

3. -21 kJ mol^-1

4. -55 kJ mol^-1

The enthalpy of formation of CO₂(g), H₂O(l) and propene (g) are -393.5, -285.8, and 20.42 kJ mol^-1 respectively. The enthalpy change for the combustion of cyclopropane at 298 K will be:

(The enthalpy of isomerization of cyclopropane to propene is -33.0 kJ mol^-1. )
1. -1021.32 kJ mol^-1
2. -2091.32 kJ mol^-1
3. -5021.32 kJ mol^-1
4. -3141.32 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. $-{273}^{\circ }C$

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. \(-169 \mathrm{~kJ} \mathrm{~mol}^{-1}\)