Given below are two statements.
Statement I: The presence of weaker $$\pi$$-bonds make alkenes less stable than alkanes
Statement II: The strength of the double bond is greater than that of carbon-carbon single bond.
In the light of the above statements, choose the correct answer from the options given below.

We need to evaluate both statements about alkenes and alkanes.

Statement I: "The presence of weaker $$\pi$$-bonds make alkenes less stable than alkanes."

The $$\pi$$ bond in alkenes is formed by the lateral overlap of unhybridized p-orbitals. This lateral overlap is less effective than the head-on overlap in $$\sigma$$ bonds, making the $$\pi$$ bond weaker and more reactive. Due to the presence of this weaker $$\pi$$ bond, alkenes are more reactive (less stable) than alkanes, which contain only strong $$\sigma$$ bonds.

Statement I is correct.

Statement II: "The strength of the double bond is greater than that of carbon-carbon single bond."

The bond energy of a C=C double bond is approximately $$614$$ kJ/mol, while the bond energy of a C-C single bond is approximately $$347$$ kJ/mol. Since $$614 > 347$$, the double bond is indeed stronger than the single bond overall (even though the $$\pi$$ component individually is weaker than a $$\sigma$$ bond).

Statement II is correct.

Note: There is no contradiction between the two statements. The double bond as a whole is stronger than a single bond, but the presence of the weaker $$\pi$$ bond component makes the molecule more reactive at that site.

The correct answer is Option A: Both Statement I and Statement II are correct.