Explanation

• Effusion is the escape of gas molecules through a tiny hole.
• According to Graham’s law, rate of effusion ∝ 1/√molar mass.
• Lighter gases effuse faster than heavier gases.
• Among given options, hydrogen has the lowest molar mass (H₂ = 2 g/mol).
• Therefore, it moves and escapes the fastest.

Last verified on 19-05-2026

Explanation

• Vapour pressure depends on the tendency of liquid molecules to escape into vapour.
• When temperature increases, molecules gain kinetic energy.
• More molecules escape from liquid phase into vapour phase.
• This increases the vapour pressure at equilibrium.
• Pressure applied from outside does not increase vapour pressure directly.

Last verified on 20-05-2026

Explanation

• Boiling point depends on intermolecular forces.
• Stronger forces require more energy to separate molecules.
• Water (H₂O) forms strong hydrogen bonding between molecules.
• H₂S has only weak van der Waals (no effective hydrogen bonding).
• Therefore, water has a much higher boiling point.

Last verified on 20-05-2026

Explanation

• A supercritical fluid forms above critical temperature and pressure.
• In this state, substance shows properties of both liquid and gas.
• It can diffuse like a gas and dissolve substances like a liquid.
• The liquid and gas phases become indistinguishable.
• Therefore, no clear boundary exists between them.

Last verified on 19-05-2026

Explanation

• A 3-center 2-electron (3c–2e) bond involves three atoms sharing two electrons.
• This type of bonding occurs in electron-deficient compounds.
• Diborane (B₂H₆) is a famous example of such bonding.
• It contains two bridging hydrogen atoms between boron atoms.
• These bridges form banana-shaped 3c–2e bonds.

Last verified on 19-05-2026

Explanation

• Ionization energy is energy required to remove an electron from an atom.
• Nitrogen has configuration: 1s² 2s² 2p³ (half-filled, stable).
• Oxygen has configuration: 1s² 2s² 2p⁴.
• In oxygen, one p orbital has paired electrons, causing repulsion.
• This repulsion makes electron removal easier in oxygen than nitrogen.

Last verified on 19-05-2026

Explanation

For spontaneity, use Gibbs free energy:

ΔG = ΔH - TΔS

Reaction becomes non-spontaneous when ΔG > 0.  

At the cutoff point ΔG = 0, so:

0 = ΔH - TΔS

T = ΔH / ΔS

Plug in the values. Convert ΔH to J/mol to match units:

ΔH = −40 kJ mol⁻¹ = −40000 J mol⁻¹  

ΔS = −100 J mol⁻¹ K⁻¹

T = (−40000) / (−100) = 400 K

Last verified on 19-05-2026

Explanation

• Dilution means adding more solvent (water) to a solution.
• Molar concentration depends on amount of solute per volume.
• When volume increases, molarity decreases.
• Specific conductivity depends on number of ions per unit volume.
• So both concentration and conductivity decrease on dilution.

Last verified on 19-05-2026

Explanation

• Nernst equation relates electrode potential to reaction conditions.
• It shows how potential changes away from standard conditions.
• Electrode potential depends on ion concentration (or activity).
• It also depends on temperature (T).
• So both factors influence the value of E.

Last verified on 19-05-2026

Explanation

• Bond order is calculated using Molecular Orbital Theory.
• Formula: Bond order = (Bonding electrons − Antibonding electrons) / 2
• O₂ has bond order = 2.
• O₂⁺ means one electron is removed from antibonding orbital.
• Removing antibonding electron increases bond order by 0.5.
• So, bond order of O₂⁺ = 2.5.

Last verified on 19-05-2026