The equation that represents general van't Hoff equation is 

• $\mathrm{\pi }= \frac{\mathrm{n}}{\mathrm{V}}\mathrm{RT}$

• $\mathrm{\pi }= \mathrm{nRT}$

• $\mathrm{\pi }= \frac{\mathrm{V}}{\mathrm{n}}\mathrm{RT}$

• $\mathrm{\pi }= \mathrm{nVRT}$

Calculate the work done during compression of 2 mol of an ideal gas from a volume of 1 m³ to 10 dm³ 300K against a pressure of 100 KPa

• -99 kJ

• +99 kJ

• +22.98 kJ

• -22.98 kJ

A gas will approach ideal behavior at

• Low temperature and low pressure

• Low temperature and high pressure

• High temperature and low pressure

• High temperature and high pressure

54.

Pressure of ideal and real gases at 0K are

• >0 and 0

• <0 and 0

• 0 and 0

• 0 and >0

Mixing of N₂ and H₂ from an ideal gas mixture at room temperature in a container. For this process, which of the following statement is true?

• $∆\mathrm{H} = 0; ∆{\mathrm{S}}_{\mathrm{surrounding}} = 0; ∆{\mathrm{S}}_{\mathrm{system}} = 0 \mathrm{and} ∆\mathrm{G} = -\mathrm{ve}$

• $∆\mathrm{H} = 0; ∆{\mathrm{S}}_{\mathrm{surrounding}} = 0; ∆{\mathrm{S}}_{\mathrm{system}} > 0 \mathrm{and} ∆\mathrm{G} = -\mathrm{ve}$

• $∆\mathrm{H} > 0; ∆{\mathrm{S}}_{\mathrm{surrounding}} = 0; ∆{\mathrm{S}}_{\mathrm{system}} > 0 \mathrm{and} ∆\mathrm{G} = -\mathrm{ve}$

• $∆\mathrm{H} < 0; ∆{\mathrm{S}}_{\mathrm{surrounding}} > 0; ∆{\mathrm{S}}_{\mathrm{system}} < 0 \mathrm{and} ∆\mathrm{G} = -\mathrm{ve}$

Consider a fuel cell supplied with 1 mol of H₂ gas and 10 moles of O₂ gas. If fuel cell is operated at 9.63 mA current, how long will it deliver power? (Assume 1 F = 96500 C/mole of electrons).

• 1 × 10⁶ s

• 0.5 × 10⁶ s

• 2 × 10⁶ s

• 4 × 10⁶ s

Critical density of a gas having molecular weight 39 g mol^-1 is 0.1 × 10³ g cm^-3. Its critical volume in L mol^-1 is

• 0.390

• 3.90

• 0.039

• 39.0

18 g of glucose is dissolved in 178.2 g of water. The vapour pressure of the solution at 100° C is (vapour pressure of pure water at 100° C is 760 mm Hg)

• 767.6 mm Hg

• 760 mm Hg

• 752.4 mm Hg

• 725.4 mm Hg

If two moles of an ideal gas at 500 K occupies a volume of 41 L, the pressure of the gas is (R = 0.082 L atm K^-1 mol^-1)

• 2 atm

• 3 atm

• 4 atm

• 5 atm

At 273 K, the density of a certain gaseous oxide at 2 atm is same as that of dioxygen at 5 atm. The molecular mass of the oxide (in g mol^-1) is

• 80

• 64

• 32

• 160