MISSED THIS? Read Section 15.6 (Pages 656 - 661); Watch KCV 15.6, IWE 15.9. Consider this three-step mechanism for a reaction: Ch₂(g) Cl(g) + CHCk (g) Cl(g) + CCk (g) 2Cl(g) (fast) → HCl(g) +CCk (g) (slow) ky (fast) → CCL (g) k₂ Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. ▸ View Available Hint(s) ΑΣΦ | a x² Xbx A chemical reaction does not occur for this question. Submit Previous Answers X Incorrect; Try Again; 3 attempts remaining ?

MISSED THIS? Read Section 15.6 (Pages 656 - 661); Watch KCV 15.6, IWE 15.9. Consider this three-step mechanism for a reaction: Ch₂(g) Cl(g) + CHCk (g) Cl(g) + CCk (g) 2Cl(g) (fast) → HCl(g) +CCk (g) (slow) ky (fast) → CCL (g) k₂ Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. ▸ View Available Hint(s) ΑΣΦ | a x² Xbx A chemical reaction does not occur for this question. Submit Previous Answers X Incorrect; Try Again; 3 attempts remaining ?

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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Step 1: CH4(g) + Cl2(g) <--> CH3(g) + HCl(g) + Cl slow Step 2: CH3(g) + Cl2(g) --> CH3Cl(g) + Cl fast A. What is the overall reaction and rate expression for the appearance of CH3Cl (g) ? B. Use the answer in part a to write the rate expression for the change in concentration of CH3(g). C. Using the steady state approximation, give an expression for the appearance of CH3Cl(g) that does not depend on the concentration of CH3(g). (Step 1 is reversible, step 2 is not)
Consider the reaction NO2(g) + CO(g) → NO(g) + CO2(g) The mechanism it is thought to the follow is: Step 1: NO2(g) + NO2(g) → NO3(g) + NO(g) Step 2: NO3(g) + CO(g) → NO2(g) + CO2(g) Which of the following species is an intermediate?
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 × 10-10 cm³ molecule-¹.s-¹ at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k = Incorrect Convert the rate constant to units of Torr-¹.s-¹. 5.962 ×10¹7 Incorrect 2 3.208 ×10¹7 What is the order of this reaction? 0 M-¹.s Torr-g
Refer to the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g). If the reaction is second order with respect to both NO2 and CO, what happens to the reaction rate when the concentration of both reactants is doubled? O Reaction rate is also doubled O Reaction rate increases by a factor of 8 O Reaction rate increases by a factor of 16 Reaction rate increases by a factor of 32
Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. Rate = 1 A[₂0] At O Rate = O Rate - Submit Rate = -A[₂0] At Correct Part B Rate = Submit A[N₂O] At Part C A[N₂0] At A[N₂O] At Previous Answers Submit Request Answer 1 A[N₂] 2 At At In the first 13.0 s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE| ΑΣΦ Request Answer A[N₂] At 1 A[N₂] At 1/1 A[0₂] At A[0₂] At A[0₂] A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O]/At? Express your answer using two significant figures. IVE| ΑΣΦ ? M-s-1 ? M-s-1
= OKINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... At a certain temperature the rate of this reaction is second order in HI with a rate constant of 6.70M¹s¹: 2HI (g) → H₂(g) + 1₂ (g) Suppose a vessel contains HI at a concentration of 1.29 M. Calculate the concentration of HI in the vessel 0.410 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation 84°F Partly sunny Check 0 x10 Q Search 0/5 J h © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center C
Based on the following mechanism write out the rate law for the overall reaction. Also identify any catalysts or intermediates. Step 1. A + B -› C Slow Step 2. B + C -› D Fast Step 3. 2D -› E Very Fast
The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results: Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s) 1 0.00542 0.00542 0.341 2 0.00542 0.0108 0.679 3 0.0108 0.00542 0.679 4 0.0108 0.0108 1.35 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2 Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HBr(g) is 0.00861 M and that of O2(g) is 0.0123 M if the temperature is the same as that used to obtain the data shown above? _________M/s
If the following chemical reactions have the same activation energy, which of them is likely to be faster at a given temperature? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b с d A(g) + 2B(g) → AB₂(g) A(g) + B(g) + C(g) → ABC(g) AB(g) + B(g) → AB₂(g) All will proceed at the same rate
Consider this three-step mechanism for a reaction: Cl₂ (g) Cl(g) + CHCl3 (g) Cl(g) + CCl3 (g) k₂ → k3 → k4 2Cl(g) (fast) HCl(g) + CCl3(g) (slow) CCl4 (g) (fast)
10 Chlorine gas reacts with aqueous hydrogen sulfide (also known as hydrosulfuric acid) to form elemental sulfur and hydrochloric acid. Cl2(g) + H2S(aq) → S(s) + 2HCl(aq) A proposed mechanism for this reaction is Step 1 Cl2 + H2S → Cl+ + HCl + HS- Step 2 Cl + HS¯ → HCl + S (slow) (fast) Sketch a potential energy diagram for this reaction, with labels to identify activation energy, transition state, rate-determining step, and any reaction intermediate.
Reaction to produce COCl2 (phosgene) from chlorine and carbon monoxide in a gaseous stateIt is said that the mechanism of is as follows.1st step: Cl2 ⇔ 2 Cl (Fast equilibrium)2nd step: Cl + CO ⇔ COCl (Fast equilibrium)3rd step: COCl + Cl2 ⇒ COCl2 + Cl (slow)4th step: 2 Cl ⇒ Cl2 (fast)Overall reaction: CO + Cl2 ⇒ COCl2Derive the rate law of this reaction.