The rate of decomposition of acetaldehyde, CH,CHO(g), into CH,(g) and CO(g) in the presence of I,(g) at 800 K follows th rate law rate of reaction = k[CH3CHO] [I2] The decomposition is believed to occur by the two-step mechanism step 1: CH,CHO(g) + I,(g) → CH,I(g) + HI(g) + CO(g) step 2: CH,I(g) + HI(g) → CH,(g) + I,(g) Which species is the catalyst for the overall reaction? O CH;I HI CO O CH,CHO CH, Which step in the proposed mechanism is most likely the rate-limiting step?

The rate of decomposition of acetaldehyde, CH,CHO(g), into CH,(g) and CO(g) in the presence of I,(g) at 800 K follows th rate law rate of reaction = k[CH3CHO] [I2] The decomposition is believed to occur by the two-step mechanism step 1: CH,CHO(g) + I,(g) → CH,I(g) + HI(g) + CO(g) step 2: CH,I(g) + HI(g) → CH,(g) + I,(g) Which species is the catalyst for the overall reaction? O CH;I HI CO O CH,CHO CH, Which step in the proposed mechanism is most likely the rate-limiting step?

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

The gas phase decomposition of dimethyl ether at 500 °C CH3OCH3(g) → CH,(g) + H2(g) + CO(g) is first order in CH3OCH3 with a rate constant of 4.00x10-4s1. If the initial concentration of CH3OCH3 is 8.82×10-2 M, the concentration of CH3OCH3 will be M after 3301 s have passed.
O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism H₂(g) + ICI(g) - 1 HI(g) + HCl(g) k₁ 2 HI(g) + ICl(g) 1₂(g) + HCl(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, K₂, and (if necessary) the rate constants k.₁ and k-2 for the reverse of the two elementary reactions in the mechanism. Explanation Check rate = k0 = 0 k = JUL 16 L tv W MacBook Air ローロ 00 X 0- © 2023 McGraw Hill LLC. All Rights Reserved. Terms of 70
2
Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.
Given the reaction below and its reaction mechanism: 2A + 2C -> F + 2E Step 1: A + A B k1/k (fast) Step 2: B + C->D+E k2 (slow) Step 3: D+ C->E+ F k3 (fast) How many intermediates are in the reaction? If the experimentally derived rate law is rate=k'[A]²[C], what is k' equal to? (in terms of rate constants of the elementary steps) Ok,kzk3 Okk2/k1 Ok /k2 Ok2/k;k3
Give typed full explanation not a single word hand written otherwise leave it
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
The gas phase decomposition of sulfuryl chloride at 600 K SO₂Cl2₂ (g) → SO₂(g) + Cl₂(g) is first order in SO₂ C12 with a rate constant of n-¹. 2.80 × 10- -3 min If the initial concentration of SO₂Cl2 is 0.00258 M, the concentration of SO₂ Cl2 will be 0.000359 M after min have passed.
The gas phase decomposition of dinitrogen pentoxide at 335 K N205(9)- →2 NO2(g) + 2 02(g) is first order in N205 with a rate constant of 4.70x10-3 s-1. If the initial concentration of N205 is 3.65×10-2 M, the concentration of N205 will be 6.39x10-3 M after || s have passed.
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)H20(g) + ½ O2(g) is second order in H2O2. In one experiment, when the initial concentration of H,O2 was 0.242 M, the concentration of H,O, dropped to 4.09×10 M after 23.5 seconds had passed. Based on these data, the rate constant for the reaction is M1s1.
2 NO (g) + O₂ (g) --> 2 NO2 (g) The proposed mechanism for the reaction above is 1) NO (g) + NO (g) --> N₂O2(g) 2) N₂O2 (g) + O2 (g) --> 2 NO2 (g) Write the rate law for the mechanism if the first step is fast and the second step is slow.
One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)