1.

Uncertainty principle is valid for

• Proton

• Methane

• Both (a) and (b)

• 1 µm sized platinum particles

The energy of an electron is the 3S orbital ( excited state) of H- atom is

• -1.5 eV

• -13.6 eV

• -3.4 eV

• -4.53 eV

Among the following, the molecule that will have the highest dipole movement is

• H₂

• HF

• HBr

• HCl

Which of the following pair have identical bond order?

• CN^- and NO⁺

• CN^- and O${}_2^{-}$

• CN^- and CN⁺

• NO⁺ and O${}_2^{-}$

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

Pressure of ideal and real gases at 0K are

• >0 and 0

• <0 and 0

• 0 and 0

• 0 and >0

For the process A (1, 0.05 atm, 32°C) → A (g, 0.05 atm, 32°C)

The correct set of thermodynamic parameters is

• $∆$G = 0 and $∆$S = -ve

• $∆$G = 0 and $∆$S = +ve

• $∆$G = +ve and $∆$S = 0

• $∆$G = -ve and $∆$S = 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?

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

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

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

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

In the ln K vs $\frac{1}{\mathrm{T}}$ plot of a chemical process having $∆$S° > 0 and $∆$H° < 0, the slope is proportional to (where K is equilibrium constant).

• -|$∆$H°|

• |$∆$H°|

• $∆$S°

• -$∆$S°

For the process,

$\frac{3}{2}$A → B, at 298 K, $∆$G° is 163 kJ mol^-1. The composition of the reaction mixture is [B] = 1 and [A] = 10000. Predict the direction of the reaction and the relation between reaction quotient (Q) and the equilibrium constant (K).

• Forwards direction because Q > K

• Reverse direction because Q > K

• Forward direction because Q < K

• Reverse direction because Q < K