lowing reaction was found experimentally to have the rate law, vok[H₂][ICI]. H-21C1-12+2HCI Two mechanisms have been proposed: k₁ H₂ + Cl₂-2 2HC1 Step 1 Step 2 HI+HCI Step 1 Mechanism 1 HI+1C-21₂2HCI Step 2 Which of the proposed mechanisms is consistent the experimental observations, given the conditions indicated below? Mechanism 2 A) Mechanism 1, where Step 2 is fast and Step 1 is slow. B) Neither mechanism is consistent with the observed rate law, C) Mechanism 2, where Step 1 is a fast, reversible step and Step 2 is slow. D) Mechanism 2, where Step 2 is fast and Step 1 is slow. E) Mechanism 1, where Step 1 is a fast, reversible step and Step 2 is slow, E

lowing reaction was found experimentally to have the rate law, vok[H₂][ICI]. H-21C1-12+2HCI Two mechanisms have been proposed: k₁ H₂ + Cl₂-2 2HC1 Step 1 Step 2 HI+HCI Step 1 Mechanism 1 HI+1C-21₂2HCI Step 2 Which of the proposed mechanisms is consistent the experimental observations, given the conditions indicated below? Mechanism 2 A) Mechanism 1, where Step 2 is fast and Step 1 is slow. B) Neither mechanism is consistent with the observed rate law, C) Mechanism 2, where Step 1 is a fast, reversible step and Step 2 is slow. D) Mechanism 2, where Step 2 is fast and Step 1 is slow. E) Mechanism 1, where Step 1 is a fast, reversible step and Step 2 is slow, E

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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Determine the rate law for the reaction, 2IC1 + H2 = I, + 2HCi, from the following initial rate data: Initial Rate(Ms') 2.04x102 4.08x102 2.55x103 5.09x103 [H,], [ICI], 0.250 0.500 0.500 0.500 0.125 0.125 0.125 0.250 A) R = k[IC1]? В) R = k[H2]? C) R = k[ICI][H_]? D) R = k[ICl][H,] E) R = k[ICI]°[H¿] 000
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[4] The reaction: 21 (aq) + S2O;²-(aq) → I½(aq) + 2SO,²-(aq) is first order with respect to I and first order with respect to S20g. The rate constant k was determined at different temperatures and a plot of In(k) versus 1/T was constructed resulting in the straight line: y = -5781.8x + 14.1. Assume k has units of M's. (a) Determine the activation energy for this reaction. (b) Calculate the value of k at 20 °C.
A certain first-order reaction has a rate constant of 2.60 x 10-2s¹ at 18 °C. What is the value of k at 55 °C if Ea = 83.5 kJ/mol? Express your answer in reciprocal seconds to three significant figures. ΨΕ ΑΣΦ Par Esc Another first-order reaction also has a rate constant of 2.60 x 10-2s¹ at 18 °C. What is the value of k at 55 °C if E2 = 130 kJ/mol? Express your answer in reciprocal seconds to three significant figures. ΕΠΙ ΑΣΦΑ Type here to search Q Z 2 W S X F3 # ? 3 ? E D 8-1 t 8-1 F4 $ 4 C F5 R F % 5 V F6 T G 6 DELL F7 B & H 14 * 8 N D 8 F10 M
the reaction and rate law for the gas phase decomposition ofdinitrogen pentaoxide are 2N205(g)--->4NO2(g) +O2(g) rate= k[N205] which of the following can be considered valid mechanisms forthe reaction? I) one-step collision II) 2N2O5(g)--->2NO3(g) +2NO2(g) [slow] 2NO3(g)--->2NO2(g) +20(g) 20(g)--- >02(g) [fast] III) N205(g)NO3(g) +NO2(g) [fast] NO2(g) + N2O5(g) ---> 3NO2(g)+ O(g) [slow] NO3(g) + O(g)---> NO2(g) +O2(g) [fast] IV) 2N2O5(g) 2NO2(g) + [fast] N203(g)+30(g) [fast] N203(g) + O(g)--- >2NO2(g) 20(g)--- >O2(g) V)2N2O5(g)--- >N4010(g) +02(g) [slow] N4010(g)---> 4NO2(g) [fast] [fast] [slow]
The enzyme carbonic anhydrase catalyzes the reactionCO2(g) + H2O(l)--->HCO3- (aq) + H+(aq). In water,without the enzyme, the reaction proceeds with a rateconstant of 0.039 s-1 at 25 °C. In the presence of the enzymein water, the reaction proceeds with a rate constantof 1.0 x 106 s-1 at 25 °C. Assuming the collision factor isthe same for both situations, calculate the difference inactivation energies for the uncatalyzed versus enzymecatalyzedreaction.
She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: (W) [200³H] 2 1.5- 0.5 0 0 t(s) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in 11/2 = ☐ s S ☐ x10 H2CO3. Calculate the value of the rate constant k. k = ☐ Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H2CO3 in the engineer's reaction vessel after 5.0 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H2CO3. Round your answer to 2 significant digits. [H₂CO,] = M
16) The reaction (C2H5)2(NH2) + 12 (C2H5)2(N2) + 2HI gives the following data. Expt Initial(C2H5)2(NH2) mol L-1 Initial 12 mol L-1 Initial rate of formation of (C2H5)2(N2) mol L-1min-1 1 0.015 0.015 3.15 x 10-1 2 0.015 0.045 9.45x 10-1 3 0.030 0.045 18.9 x 10-1 a) Determine the order of the reaction with respect to each reactant. Explain how you arrived at each answer. (Show your method) b) What is the overall order of the reaction? c) Write the rate law expression. d) Calculate the rate constant, k and provide the proper units. e) If (C2H5)2(N2) is formed at a rate of 9.45 M/s in experiment 3, what is the rate of appearance of HI? f) In experiment 3, assuming it goes to completion, if all of [(C2H5)2(NH2) ] is reacted, what would be the amount of 12 remaining?
Please provide proper explanation of the concept and solution
The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
At a certain temperature the rate of this reaction is first order in N₂O5 with a rate constant of 0.0125 s¯¹: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) Suppose a vessel contains N₂O5 at a concentration of 1.14M. Calculate the concentration of N₂O5 in the vessel 88.0 seconds later. You may assume no of reaction is important. Round your answer to 2 significant digits.
Give a reaction rate for the provided mechanism and do not include the intermediates in the final equation. 1. For the spontaneous reaction in water: Re(HzO)z + 2 KCN →Re(CN)z2 + 2K*(aq) + 2 H2O The postulate mechanism is where all species are in aqueous phase k1 Re(H₂O)2 + CN- Re(H₂O)(CN) + H₂O equilibrium Re(H₂O)(CN) + CN-I2 Re(H₂O)(CN)2-² Re(H2O)(CN)2243 Re(CN)22 + H2O k2 slow fast