If the reaction X + 2 Y → XY₂ occurs by the proposed mechanism, what is the rate law? Step 1 X + Y ⇌ XY (slow) Step 2 XY + Y → XY₂ (fast) A rate = k[X] B rate = k[Y] C rate = k[Y]² D rate = k[X][Y] E rate = k[X][Y]²
Added by Charles D.
Close
Step 1
The rate law is determined by the slowest step in the reaction mechanism. The given mechanism is: Step 1: X + Y ⇌ XY (slow) Step 2: XY + Y → XY₂ (fast) The slow step is Step 1: X + Y ⇌ XY. Show more…
Show all steps
Your feedback will help us improve your experience
Anil Kumar Singh and 66 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
In hypothetical reaction $\mathrm{X}_{2}+\mathrm{Y}_{2} \rightarrow 2 \mathrm{XY}$ Follows the mechanism as given below $\mathrm{X}_{2}=\mathrm{X}+\mathrm{X}$ (fast reaction) $\mathrm{X}+\mathrm{Y}_{2} \rightarrow \mathrm{XY}+\mathrm{Y}$ (slow reaction) $\mathrm{X}+\mathrm{Y} \rightarrow \mathrm{XY}$ (fast reaction) Here the correct statement is/are a. Order of reaction is $3 / 2$. b. Molecularity is 2 . c. $\mathrm{R}=\mathrm{k}[\mathrm{X}]\left[\mathrm{Y}_{2}\right]$ d. Both molecularity and order $=3$
A gaseous reaction occurs by a two-step mechanism, shown below: Step 1: AX + Y2 ⇌ AXY2 (fast) Step 2: AXY2 + AX → 2 AXY (slow) Including concentration of only reactants and products, what is the rate law for this reaction? Rate = k[AXY2]/[AX][Y2] Rate = k[AX]2[Y2] Rate = k[AX][XY2] Rate = k[AXY]2/[A Y2][AX]
Adi S.
A reaction mechanism has the following proposed elementary steps: Step 1: A ⇌ B + C Step 2: A + B → D Step 3: 2 A + D → C + E If Step 2 is the rate-limiting step, what would the proposed rate law for this mechanism be? A) Rate = k[A] B) Rate = k[A]²[D] C) Rate = k[A]⁴ D) Rate = k[A][B] E) Rate = k[A]²/[C]
Madhur L.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD