An ideal gas can be expanded from an initial state to a certain volume through two different processes,
(A) $P{V}^2=K$ and (B) $P=K{V}^2$, where K is a positive constant.

Choose the correct option based on the above statement:

1. Final temperature in (A) will be greater than in (B)

2. Final temperature in (B) will be greater than in (A)

3. Work done by the gas in both the processes would be equal

4. Total heat given to the gas in (A) is greater than in (B)

Heat of hydrogenation of ethene is x₁ and that of benzene is x₂. Hence resonance energy is-

1. $x_1-x_2$

2. $x_1+x_2$

3. $3x_1-x_2$

4. $x_1-3x_2$

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

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. $x_1{T}_1+x_2+x_3-x_4$

Which of the following is the enthalpy change for the hydrogenation of ethyne to ethene?

HC≡CH + H₂ → C₂H₄
Given bond energies: 
C≡C = 198 kcal mol⁻¹
C–H = 98 kcal mol⁻¹
H–H = 103 kcal mol⁻¹
C=C = 145 kcal mol⁻¹

1. 48 kcal

2. 96 kcal

3. -40 kcal

4. -152 kcal

$H_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\to H_{2}O\left(l\right)$

B.E. (H-H) = x₁; B.E. (O=O) = x₂ B.E. (O-H) = x₃

Latent heat of vaporization of water liquid into water vapour = x₄, then $∆H_f$(heat of formation of liquid water) is:

1. $x_1+\frac{x_2}{2}-x_3+x_4$

2. $2x_3-x_1-\frac{x_2}{2}-x_4$

3. $x_1+\frac{x_2}{2}-2x_3-x_4$

4. $x_1+\frac{x_2}{2}-2x_3+x_4$

During a process, the pressure of a gas is inversely proportional to the square of its volume. If the temperature of the gas increases, the work done on the gas is:
1. Positive
2. Negative
3. Zero
4. May be positive or negative

For the following reaction:
\(𝐶 𝑂_ 2 (𝑔) + 𝐶 (𝑠) → 2 𝐶 𝑂 (𝑔)\);  \(\Delta H^\circ = 172.5\text{ kJ}\)
The standard enthalpies of formation of CO₂(g) and CO(g) at 298 K are in the ratio 2.57 : 1.

What is the standard enthalpy of formation (\(\Delta H_f^\circ\)) of CO(g)?
1. -150.6 kJ mol^-1

2. -302.63 kJ mol^-1

3. -130.2 kJ mol^-1

4. -141.8 kJ mol^-1

In an adiabatic expansion the product of pressure and volume-

1. decreases

2. increases

3. remains constant

4. first increase then decreases

The molar entropy of vaporization of acetic acid at its boiling point, 118°C, is 14.4 cal K⁻¹ mol⁻¹. Calculate the latent heat of vaporization of acetic acid in cal g⁻¹.

100 ml of 0.3 M HCl solution is mixed with 100 ml of 0.35 M NaOH solution. The amount of heat liberated is

1. 7.3 kJ

2. 5.71 kJ

3. 10.42 kJ

4. 1.713 kJ