(A): The C-C bond length in benzene is intermediate between C-C single bond length and C-C double bond length.(R): Benzene molecule exhibits resonance (A) Both (A) and (R) are true and (R) is the correct explanation of (A)(B) Both (A) and (R) are true and (R) is not the correct explanation of (A)(C) (A) is true but (R) is false(D) (A) is false but (R) is true

The correct answer is:

(B) Both (A) and (R) are true, but (R) is not the correct explanation of (A).

Explanation:

(A) The C-C bond length in benzene is intermediate between C-C single bond length and C-C double bond length.
This statement is true. In benzene, the carbon atoms are bonded in a planar hexagonal ring, and the bonds between the carbon atoms are actually a combination of single and double bonds. The electron density in the carbon-carbon bonds is spread out over all six carbon atoms due to resonance, leading to an intermediate bond length between that of a single bond and a double bond.

(R) Benzene molecule exhibits resonance.
This statement is true. Benzene is a classic example of a molecule that exhibits resonance. The electrons in the carbon-carbon bonds are delocalized, meaning they are not localized to a specific single or double bond but are spread out across the entire ring. This results in the stability of the molecule and the equalization of the bond lengths and bond strengths.

However, while both statements (A) and (R) are true, (R) is not the correct explanation of (A). The intermediate bond length in benzene is a result of resonance, where the electrons are delocalized, leading to an equal distribution of bond lengths, rather than resonance being the explanation for the intermediate bond length. Therefore, the correct answer is (B).