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

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

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)

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?

The entropy change in the conversion of one mole of liquid water at 373 K to vapour at the same temperature would be: (Latent heat of vaporization of water, $∆H_{vap}=2.257$ $kJ/g$)

1. 105.9 JK^-1mol^-1

2. 107.9 JK^-1mol^-1

3. 108.9 JK^-1mol^-1

4. 109.9 JK^-1mol^-1

Which of the following is the correct sign of entropy change (ΔS) for the conversion:

C(graphite) → C(diamond)

1. Zero

2. Positive

3. Negative

4. Cannot be determined from given data

To calculate the amount of work done in joules during reversible isothermal expansion of an ideal gas, the volume must be expressed in:

Which of the following conditions will always lead to a non-spontaneous change?

1. Positive $∆H$ and positive $∆S$

2. Negative$∆H$ and negative $∆S$

3. Positive $∆H$ and negative $∆S$

4. Negative $∆H$ and positive $∆P$

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.