The overall reaction 2A + 2B = D+ E takes place in two steps: STEP 1 (fast): A + 2B = C STEP 2 (slow): C + A D+E What is the rate law for this process? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a RATE = k[A] [B}? b RATE = k[A][C] RATE = k(A][B]? RATE = k[A][B]

The overall reaction 2A + 2B = D+ E takes place in two steps: STEP 1 (fast): A + 2B = C STEP 2 (slow): C + A D+E What is the rate law for this process? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a RATE = k[A] [B}? b RATE = k[A][C] RATE = k(A][B]? RATE = k[A][B]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Answer in two significant digits, please!
The reaction A + 2B → products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. By what factor does the rate of reaction increase? 3 fold 6 fold 9 fold 27 fold the rate of reaction does not change with a change in the [B].
Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center
3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
just need standard error for K
A2 -> 2A (slow) 2A + B2 -> 2AB (fast) What is the rate law for the overall reaction?
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
Consider this reaction: 2H1 (g) → H₂(g) +1₂(e) At a certain temperature it obeys this rate law. rate = (0.345-¹) [HI] Suppose a vessel contains HI at a concentration of 0.730M. Calculate how long it takes for the concentration of HI to decrease by 86.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. 08
A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)
Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2HI (g) - H, (g) +L, (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time [HI] (milliseconds) 0.100 M 10. 0.0494 M 20. 0.0328 M 30. 0.0245 M 40. 0.0196 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k I Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above