Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast) Cl2(g) = 2 CI(g) (2 - slow) CI(g) + CHCI3(g) HCI(g) + CCI3(g) --> (3 - fast) CI(g) + CCI3(g) --> A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect? %3D (Choose the best answer.) The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3). Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove reaction equation may be in the reaction rate law.

Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast) Cl2(g) = 2 CI(g) (2 - slow) CI(g) + CHCI3(g) HCI(g) + CCI3(g) --> (3 - fast) CI(g) + CCI3(g) --> A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect? %3D (Choose the best answer.) The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3). Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove reaction equation may be in the reaction rate law.

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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Consider the following mechanism for the oxidation of carbon monoxide:
For the reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibriumNOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibriumN2O2 + Cl2 2NOCl slow Cl2 2Cl slowCl + NO NOCl fast NO + Cl2 NOCl + Cl slowCl + NO NOCl fast
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Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88
mechanism 1 overall reaction is 2NO + Cl2 --> 2NOCl NO + Cl2 = NOCl2 fast equilibriumNOCl2 + NO---> 2NOCl slow rate law for mechanism 1 is rate=k[no2]^2[cl2] mechanism 2 Cl2 --> 2Cl slowCl + NO --> NOCl fast rate law for this mechansim 2 is rate=k[cl2] i noticed that when the mechanism has a fast reaction at equilibrium, the rate law includes reactants form both fast and slow, whereas when the reaction has fast reactions not at equilibrium, the rate law is only the reactants from the slow step (rate determining step) why is the rate law different when the fast reaction is at equilibrium vs when the mechansim has a fast reaction not at equilibrium?
The reaction Cl2(g) + CHCl3(g) --> CCl4(g) + HCl(g) proceeds through the following mechanism: Cl2(g) --> 2 Cl(g)Cl(g) + CHCl3(g) --> HCl(g) + CCl3(g)Cl(g) + CCl3(g) --> CCl4(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [Cl2] [CHCl3]Rate = k [Cl2]2 [CHCl3] Rate = k [Cl2] [CHCl3]2Rate = k [Cl2]1/2 [CHCl3] Rate = k [Cl2] [CHCl3]1/2 Rate = k [Cl2]2 Rate = k [Cl2]2 [CHCl3]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [Cl2] [CHCl3] Rate = k [Cl2]2 [CHCl3] Rate = k [Cl2] [CHCl3]2 Rate = k [Cl2]1/2 [CHCl3] Rate = k [Cl2] [CHCl3]1/2 Rate = k [Cl2]2 Rate = k [Cl2]2 [CHCl3]1/2 Rate = k [Cl2]
) In studying this reaction, the following mechanism is proposed. k1 A + B C* + B* k2 A + B* C* K3 C* + B D + B* K4 20* → E (product) Find the rate law for the consumption of A. (Assume that k4>>k₁ and k4>>k3).
Give IUPAC for the following compound = Strategy: Remember the following rule; If the alkyl substituent has six or more than six carbons, the compound is named as phenyl-substituted alkane. If the alkyl substituent has less than six carbons, the hydrocarbon is named as an Alkyl-substituted benzenes. Then, select the longest carbon chain giving lowest possible numbers for its substituents. In this particular case, either side we get 2 and 5 numbers for the substutuents. Then how we select which way we should number? Now we need to think about the alphabet order, the substituents are methyl and phenyl, therefore methyl should have the lowest possible number as M comes first in the alphabet.