elementary reactionrate constantN₂O(g) → N₂(g) + O(g)-k₁2 N₂0(g) + O(g) N₂(g) + O₂(9)k₂.Suppose also k₁k2. That is, the first step is much faster than the second.1Pate law implied by a simple mechanismWrite the balancedchemical equation for theoverall chemical reaction:Write the experimentally-observable rate law for theoverall chemical reaction.Note: your answer shouldnot contain theconcentrations of anyintermediates.Express the rate constantk for the overall chemicalreaction in terms of k₁, K₂,and (if necessary) the rateconstants k.1 and k-2 forthe reverse of the twoelementary reactions inthe mechanism.ExplanationCheck0rate = kk =JULtvWXローロ On004PH© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce Some measurements of the initial rate of a certain reaction are given in the table below.[H₂] [₂] initial rate of reaction2.44M 0.639M56.0M/s2.44M 0.154M13.5M/s7.70M 0.639 M177.M/sUse this information to write a rate law for this reaction, and calculate the value of the rate constant k.Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.rate = kk=ExplanationCheckJUL16x100.0x00StvW2023 McGraw Hill LLC. All Rights Reserved.Terms of Use

We have to find overall, rate and rate constant values.

1 hentary reaction N₂0(g) → N₂(g) + O(g) - k₁ N₂(g) + O₂(g) k₂. Suppose also k₁k₂. That is, the first step is much faster than the second. 2 N₂0(g) + O(g) 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 1 Check 0 rate = k rate constant k = olo X S

1 hentary reaction N₂0(g) → N₂(g) + O(g) - k₁ N₂(g) + O₂(g) k₂. Suppose also k₁k₂. That is, the first step is much faster than the second. 2 N₂0(g) + O(g) 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 1 Check 0 rate = k rate constant k = olo X S

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

Consider this reaction: CICH,CH,CI (g) → CH,CHCI (g) +HCI (g) At a certain temperature it obeys this rate law. rate = (0.00421 s*)[CICH,CH,CI] S Suppose a vessel contains CICH,CH,Cl at a concentration of 1.13 M. Calculate how long it takes for the concentration of CICH,CH,Cl to decrease by 85.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. ?
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
Suppose also k₁<
The reaction between N2O5 and water$$N2O5(g)+H2O(g)2HNO3(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.
20
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
Consider this reaction: 2Cl,05 (g) → 2C1, (g) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.0272 Ms)[ci,037² -1 'S Suppose a vessel contains Cl,O, at a concentration of 0.300M. Calculate how long it takes for the concentration of Cl,O, to decrease to 20.0% of its initial 5. value. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
Please don't provide handwritten solution .....
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
You are studying the reaction A₂(g)+B₂(g) →2AB(g) to determine its rate law. Assuming that you have a valid exper-imental procedure for obtaining [A₂] and [B₂] at various times,explain how you determine (a) the initial rate, (b) the reaction orders, and (c) the rate constant.
Consider the following reaction: A + B + C → D The rate law for this reaction is as follows: [A][C]* Rate = k [B]L/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.17x10-2 mol · L-ls¬1. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Templates Symbols uado redo reset keyboard shortcuts help Rate = mol · L-!s-1