Consider the following reaction,

S + O₂ $\to$ SO₂,  $∆$H = – 298.2 kJ mole^–1

SO₂ + 1/2 O₂ $\to$  SO₃, $∆$H = – 98.7kJ mole^–1

SO₃ + H₂O $\to$ H₂SO₄ , $∆$H = – 130.2 kJ mole^–1

H₂ + 1/2 O₂ $\to$ H₂O, $∆$H = – 287.3 kJ mole^–1

the enthalpy of formation of H₂SO₄ at 298 K will be–

1.	– 814.4 kJ mole–1	2.	+ 814.4 kJ mole–1
3.	– 650.3 kJ mole–1	4.	– 433.7 kJ mole–1

2.1 g of Fe combines with S evolving 3.77 kJ. The heat of formation of FeS in kJ/mole is–

Pairs correctly represent intensive property among the following is:

1. Entropy, Gibb’s energy

2. Enthalpy, Heat capacity

3. Electrode potential, Vapour pressure

4. Resistance, Conductance

An ideal gas is expanded irreversibly against 10 bar pressure from 20 litres to 30 litres. Calculate 'w' if the process is isoenthalpic.

The standard enthalpy of combustion at ${25}^{\circ }C$ of hydrogen, cyclohexene (C₆H₁₀), and cyclohexane (C₆H₁₂) are -241, -3800 and -3920 kJ mol^-1, respectively. Calculate the standard enthalpy of hydrogenation of cyclohexene.

4.8 g of C(diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of the formation of gaseous carbon is 725 kJ/mol. The energy required for the given process will be:

(i) $\mathrm{C}\left(\mathrm{graphite}\right)\to \mathrm{C}\left(\mathrm{gas}\right)$

(ii) $\mathrm{C}\left(\mathrm{diamond}\right)\to \mathrm{C}\left(\mathrm{gas}\right)$

As an isolated box, equally partitioned, contains two ideal gasses A and B as shown:

When the partition is removed, the gases mix. The changes in enthalpy $(∆\mathrm{H})$ and entropy $(∆\mathrm{S})$ in the process, respectively, are

1. Zero, positive

2. Zero, negative

3. Positive, zero

4. Negative, zero

The $∆\mathrm{H}$ for vaporization of a liquid is \(20 \mathrm{~kJ} / \mathrm{mol}.\) Assuming ideal behaviour, the change in internal energy for the vaporization of \(1 \mathrm{~mol}\) of the liquid at \(60^{\circ} \mathrm{C}\) and 1 bar is close to:

The entropy change in the isothermal reversible expansion of 2 moles of an ideal gas from 10 to 100 L at 300 K is

1. $42.3 \mathrm{J} {\mathrm{K}}^{-1}$

2. $35.8 \mathrm{J} {\mathrm{K}}^{-1}$

3. $38.3 \mathrm{J} {\mathrm{K}}^{-1}$

4. $32.3 \mathrm{J} {\mathrm{K}}^{-1}$

An ideal gas expands isothermally from ${10}^{-3}{m}^3 to {10}^{-2} m^3$ at 300 K against a constant pressure of ${10}^5 N{m}^{-2}$. The work done by  the gas is: