Suppose that the gas-phase reaction A B and B A are both elementary processes wi

Question

Suppose that the gas-phase reaction A B and B A are both elementary processes with rate constants of 6.56e-02 s-1 and 3.51e-04 s-1, respectively. Figure out the value of the equilibrium constant, KP, for the equilibrium A(g) B(g), and figure out which of the two substances, A or B develops higher partial pressure at equilibrium. Use this information to pick the choice from below which is correct.



a) KP = 1.87e+02, and B(g) develops higher partial presssure.
b) KP = 6.52e-02, and A(g) develops higher partial presssure.
c) KP = 5.35e-03, and A(g) develops higher partial presssure.
d) KP = 5.35e-03, and B(g) develops higher partial presssure.
e) KP = 1.87e+02, and A(g) develops higher partial presssure.

Explanation / Answer

The answer is: a) KP = 1.24e-01, and A(g) develops higher partial presssure.

A(g) <=> B(g)

Rate constant of forward reaction = k1 = 5.40 x 103 s-1

Rate constant of reverse reaction = k-1 = 4.35 x 104 s-1

At equilibrium, forward rate = reverse rate

k1 x P(A) = k-1 x P(B)

Equilibrium constant Kp = P(B)/P(A)

= k1/k-1

= 5.40 x 103/4.35 x 104

= 1.24 x 10-1 = 1.24e-01

P(B) = 1.24 x 10-1 x P(A)

Thus P(B) < P(A) and A(g) develops higher partial presssure

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

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