Rate law problem PLEASE SHOW ALL WORK Incorrect 0/1.5 pts Question 10 onsider th

Question

Rate law problem

PLEASE SHOW ALL WORK

Incorrect 0/1.5 pts Question 10 onsider the overall reaction: AB(g) + CB(g)A(g) + CB2(g) A proposed mechanism for this reaction is 2 AB(g) AB2(g) + A(g) (fast) AB2(g) + CB(g)Ag) + CB2(g) (slow) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in terms of k and the necessary concentrations (ex: k[XI[YIA2). Use brackets around the concentrations and the caret symbol prior to the exponent. Do not include any multiplication or division signs. Type in subscripts as normal numbers (ex: AB2, CB2) Rate = k[AB]A(2)[A]A(-1)[CB]

Explanation / Answer

rate depends on the slowest step

here 2nd step is slowest

So,

rate = k2[AB2][CB]

But AB2 is intermediate. We will be removing it using step 1

Kc = [AB2][A] / [AB]^2

[AB2] = Kc[AB]^2/[A]

[AB2] = Kc[AB]^2[A]^-1

put this in rate equation:

rate = k2[AB2][CB]

rate = k2Kc[AB]^2[A]^-1[CB]

write k2*kc as k

rate law is:

rate = k [AB]^2[A]^-1[CB]

Related Questions

Navigate

• Browse (All)
• Browse R
• Subjects

---

---

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