(A) : Viscosity of H₂O₂ < Viscosity of H₂O
(R) : Extent of H-bonding in H₂O₂ is lesser than extent H-bonding in H₂O

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(A) is true but (R) is false

Both (A) and (R) are correct and (R) is the correct explanation of (A)

Both (A) and (R) are false

Both (A) and (R) are correct but (R) is not the correct explanation of (A)

answer is D.

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Detailed Solution

Viscosity is a measure of a fluid's resistance to flow, and it is determined by the intermolecular forces between the molecules of the fluid.
The stronger the intermolecular forces, the higher the viscosity.
H₂O₂ has a bent molecular shape, which results in weaker intermolecular forces than H₂O, which has a linear molecular shape.
However, H₂O₂ is a larger molecule than H₂O, and it has more complex intermolecular interactions, including hydrogen bonding, van der Waals forces, and dipole-dipole interactions.
These interactions lead to a higher viscosity for H₂O₂ compared to H₂O.
Every water molecule can form a maximum of four hydrogen bonds.
Two hydrogen bonds are formed through two lone pairs of the oxygen atom in water and one each from the two hydrogen atoms as shown in the figure.

Each molecule of H₂O₂ can form a maximum of two hydrogen bonds.
H₂O₂ has two O-H bonds, and each of these can potentially form a hydrogen bond with a neighboring molecule.
However, the bent molecular shape of H₂O₂ means that the orientation of the O-H bonds is not ideal for maximum hydrogen bonding interactions.
As a result, H₂O₂ has weaker intermolecular forces compared to H₂O, which has a linear shape and can form up to four hydrogen bonds with neighboring water molecules.
So, Both (A) and (R) are false.