onsider this reaction: 2503 (g) → 2S0, (g)+ )+O2(g) ta certain temperature it obeys this rate law. - (4.8 5")[so,] rate = (4.8 s uppose a vessel contains SO, at a concentration of 1.42M. Calculate how long it takes for the concentration of SO, to decrease to 0.071M. You may assume o other reaction is important. ound your answer to 2 significant digits.

onsider this reaction: 2503 (g) → 2S0, (g)+ )+O2(g) ta certain temperature it obeys this rate law. - (4.8 5")[so,] rate = (4.8 s uppose a vessel contains SO, at a concentration of 1.42M. Calculate how long it takes for the concentration of SO, to decrease to 0.071M. You may assume o other reaction is important. ound your answer to 2 significant digits.

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...

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9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I¯(aq). What is the rate law for this reaction? Step 2 (fast) H₂O2(aq) + 10 (aq) → H₂O(l) + O2(g) + (aq) A) rate= K[H₂O₂] B) rate= K[H₂O₂]² C) rate= K[H₂O₂] [1] D) rate = K[H₂O₂] [10] E) rate = K[H₂O₂]²[1]/[H₂O] Tap here or pull up for additional resources 36% Submit
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Consider this reaction: 2C1,0, (g) → 2C1, (g) + 50, (g) At a certain temperature it obeys this rate law. (3,3 5")[CL0;] rate = Suppose a vessel contains Cl,0, at a concentration of 0.240M. Calculate how long it takes for the concentration of Cl,0, to decrease to 8.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
just the part in red, I listed the options too. (:
Consider the following equation: H2CO3 (aq) → H2O (l) + CO2 (g) Rate = k [HCO3-]2 Rate = - ∆ [CO2]/ 2 ∆t Rate =k [CO2]n Rate = ∆ [H2O]/ ∆t Rate = -k (∆[H2CO3]/ (3 ∆t)