Which of the given reactions has an equilibrium constant more favorable to the r

Question

Which of the given reactions has an equilibrium constant more favorable to the right? Explain your reasoning: Both carbocations are very unstable, so the equilibrium constants for both reactions are equal. The fluorine substituent's can stabilize the positive charge. Due to this stabilization, the energy of the cation in the Reaction 2 is smaller, therefore, the equilibrium constant for its formation is larger. The fluorine substituent's destabilize the positive charge. The energy of the cation in the Reaction 2 is larger, therefore, the equilibrium constant for its formation is smaller. Both equilibriums are shifted to the left, so we cannot compare the equilibrium constants.

Explanation / Answer

A) i) Reaction 1 has equilibrium more favorable to right.

ii) The fluorine substituents destabilize the positive charge.The energy of the cation in the reaction 2 is larger, therefore, the equilibriumconstnat for its formation is smaller.

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.