For the reaction, 2Cl(g) $\to$ Cl₂(g), the correct option is:

1.	\(\Delta_{\mathrm{r}} \mathrm{H}>0\) and \(\Delta_{\mathrm{r}} \mathrm{S}<0 \)	2.	\(\Delta_{\mathrm{r}} \mathrm{H}<0\) and \( \Delta_{\mathrm{r}} \mathrm{S}>0 \)
3.	\(\Delta_{\mathrm{r}} \mathrm{H}<0 \) and \(\Delta_{\mathrm{r}} \mathrm{S}<0 \)	4.	\(\Delta_{\mathrm{r}} \mathrm{H}>0\) and \( \Delta_{\mathrm{r}} \mathrm{S}>0\)

What is the value of ∆H for the reaction 2Al + Cr₂O₃ → 2Cr + Al₂O₃, knowing that the enthalpies of
formation of Al₂O₃ and Cr₂O₃ are –1596 kJ and –1134 kJ, respectively?

Plants and living beings are examples of:
1. Isolated system
2. Adiabatic system
3. Open system
4. Closed system

Identify the false statement among the following.

Assume each reaction is carried out in an open container. For which of the following reactions will 
∆ H be equal to ∆ U ?

1. ${\mathrm{PCl}}_3\left(\mathrm{g}\right)$ $\to {\mathrm{PCl}}_3\left(\mathrm{g}\right)$ $+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$ $$

2. $2\mathrm{CO}\left(\mathrm{g}\right)$ $+{\mathrm{O}}_2\left(\mathrm{g}\right)$ $\to 2{\mathrm{CO}}_2\left(\mathrm{g}\right)$ $$

3. ${\mathrm{H}}_2\left(\mathrm{g}\right)$ $+{\mathrm{Br}}_2\left(\mathrm{g}\right)$ $\to 2\mathrm{HBr}\left(\mathrm{g}\right)$

4. $\mathrm{C}\left(\mathrm{s}\right)$ $+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$ $\to 2{\mathrm{H}}_2\left(\mathrm{g}\right)$ $+{\mathrm{CO}}_2\left(\mathrm{g}\right)\hspace{0.17em}$

Which of the following is not an endothermic reaction?

1. Combustion of methane

2. Decomposition of water

3. Dehydrogenation of ethane or ethylene

4. Conversion of graphite to diamond

Find the condition under which the standard Gibbs free energy change, ΔG°, is negative.

Hydrolysis of sucrose is given by the following reaction

Sucrose + H₂O $\rightleftharpoons$ Glucose + Fructose

If the equilibrium constant (K_c) is 2$\times$10¹³ at 300 K, the value of ${∆}_r{G}^{⊝}$ at the same temperature will be:

1. 8.314 J mol^–1 K^–1$\times$300 K$\times$ln (2$\times$10¹³)

2. 8.314 J mol^–1 K^–1$\times$300 K$\times$ln (3$\times$10¹³)

3. –8.314 J mol^–1 K^–1$\times$300 K$\times$ln (4$\times$10¹³)

4. –8.314 J mol^–1 K^–1$\times$300 K$\times$ln (2$\times$10¹³)

\(\underset {-10.7 \mathrm{JK}^{-1}{mol}^{-1}} {\mathrm{H}_{(a q)}^{+}+\mathrm{OH^{-}}_{(a q)}} \rightarrow \underset {+70 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} } {\mathrm{H}_{2} \mathrm{O}_{(l)}} ~~ \mathrm{S}^{\circ}(298 \mathrm{~K})\)

Standard entropy change for the above reaction is:

1. 60.3 JK^-1 mol^-1

2. 80.7 JK^-1 mol^-1

3. -70 JK^-1 mol^-1

4. +10.7 JK^-1 mol^-1

Calculate the entropy change when one mole of liquid water at 373 K is converted into water vapour at the same temperature.

Given: Latent heat of vaporisation of water, ΔHᵥₐₚ = 2.257 kJ g⁻¹.

1. 105.9 JK^-1mol^-1

2. 107.9 JK^-1mol^-1

3. 108.9 JK^-1mol^-1

4. 109.9 JK^-1mol^-1