Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl₂(g) → NOC1₂(9) k₁ 2 NOCI ₂(g) + NO(g) → 2 NOCI(g) k₂ Suppose also k₁k₂. That is, the first step is much faster 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. 10 rate = k k=

Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl₂(g) → NOC1₂(9) k₁ 2 NOCI ₂(g) + NO(g) → 2 NOCI(g) k₂ Suppose also k₁k₂. That is, the first step is much faster 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. 10 rate = k k=

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 reaction, 2 NO(g) + Cl2(g) --> 2 NOCl(g), proceeds through the following mechanism: NO(g) + Cl2(g) --> NOCl2(g)NOCl2(g) + NO(g) --> 2 NOCl(g) The second step of this mechanism is rate-determining (slow). What would the rate law for this reaction be if the first step were rate-determining?
In the presence of vanadium oxide, SO2 (g) reacts with anexcess of oxygen to give SO3 (g):SO2 (g) + ½ O2 (g) → SO3 (g)This reaction is an important step in the manufacture of sulfuric acid. It is observed that tripling the SO2 concentration increases the rate by a factor of 3, but tripling the SO3 concentration decreases the rate by a factor of 1.7 ≈ √3. The rate is insensitive to the O2 concentration as long as an excess of oxygen is present.(a) Write the rate expression for this reaction, and give the units of the rate constant k.(b) If [SO2] is multiplied by 2 and [SO3] by 4 but all other conditions are unchanged, what change in the rate will be observed?
Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2 NO(g) N₂O₂(9) N₂O₂(g) + O₂(g) → 2NO₂(g) step 1 2 Write the balanced chemical equation for the overall chemical reaction: Suppose also k₁ <
step elementary reaction rate constant 1 NO₂(g) + F₂(g) → k₁ 2 F (g) + NO₂(g) NO₂F (g) k₂ Suppose also k₁k2. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k 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. k = 0 NO₂F(g) + F(g) 0-0 믐 010 X
1
The formation of nitrosyl chloride is described by the following chemical equation: 2NO (g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Cl₂ (g) NOCI₂ (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. 11 × Ś
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.
Deducing a rate law from the change in concentration over time A chem raduate student is studying the rate of this reaction: 2N,05 (g) → 2N,0,(g)+O, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds: time (seconds) N,0s] 0.0300 M 1.0 0.0114 M 2.0 0.00707 M 3.0 0.00511 M 4.0 0.00401 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k I %3D x10 Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be sure vour answer has the correct unit svmbol. Explanation Check 2021 McGraw-Hill Education. II
Consider the hypothetical reaction A +B+ 2C → 2D + 3E where the rate law is ΔΙΑ = k[A][B]? At Rate An experiment is carried out where [A]o = 1.0 x 10-² M, [B]o 6.0 M, 2 and [C, = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mol -1 S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 19.0 seconds. Concentration M d. Calculate the concentration of C after 19 seconds. Concentration = M
Suppose the formation of iodine proceeds by the following mechanism: step elementary reaction 1 H₂(g) + IC1 (g) → HI(g) + HC1 (g) k₁ 2 HI (g) + IC1 (g) → I₂ (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. 0 rate = k rate constant
Under certain conditions the rate of this reaction is zero order in hydrogen lodide with a rate constant of 0.0038 M's ': 2 HI(g) H,(g)+1,(g) Suppose a 4.0L flask is charged under these conditions with 100, mmol of hydrogen lodide. After how much time is there only 50.0 mmol left? You may assume no other reaction Is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
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