For the reaction \(\text{A}_2(\text{g}) \rightleftharpoons 2\text{A}(\text{g})\) \(\Delta G^o(\text{A}_2) = -100 \, \text{kJ/mol}\) \(\Delta G^o(\text{A}) = -50.8625 \, \text{kJ/mol}\) At 300 K and 1 atm pressure, the degree of dissociation of A$_2$ gas at equilibrium is \(x \times 10^{-2}\). Find \(x\). \(\text{[R = 8.3 J/molK]}\)
Show Hint
The equilibrium constant expression for dissociation reactions can be used to determine the degree of dissociation from Gibbs free energy values.
Let P be an Alkyl Chloride and Q be Chlorobenzene (Aryl Chloride).
Analysis:
- (A) In Q, the Cl lone pair participates in resonance with the ring, acquiring a partial positive charge. In P, Cl pulls electrons via induction ($\delta^-$). So Q has *less* $\delta^-$ on Cl. (False).
- (B) Dipole moment of Chlorobenzene (Q) is lower than Alkyl Chloride (P) because the C-Cl bond moment opposes the resonance moment? Actually, $sp^2$ carbon is more electronegative than $sp^3$, reducing the bond polarity C-Cl. P has higher dipole. (False).
- (C) Resonance in Chlorobenzene creates partial double bond character in C-Cl. (True).
- (D) In Q (Chlorobenzene), C is part of benzene ring ($sp^2$). In P (Alkyl), C is $sp^3$. (True).
- (E) Partial double bond character makes the bond *shorter*, not longer. (False).
Conclusion: Only C and D are correct.
