Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism. rate constant step elementary reaction 1 NO₂(g) +03 (g) → NO₂ (g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O₂ (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. Explanation Check 0 rate= = k 0 14 Stv N 10 0-0 8 X Ⓒ2022 McGraw Hill LLC

Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism. rate constant step elementary reaction 1 NO₂(g) +03 (g) → NO₂ (g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O₂ (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. Explanation Check 0 rate= = k 0 14 Stv N 10 0-0 8 X Ⓒ2022 McGraw Hill LLC

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

A chemist conducted a study of the decomposition of phosphine gas, PH3 (g), into phosphorous gas, P4(g), and hydrogen gas. This reaction is represented by the following balanced chemical equation: 4 PH3(g) → P4(g) + 6 H2(g) She determined the rate of reaction with respect to the consumption of phosphine gas to be -0.0024 mol/(L s). What are the rates of formation of phosphorous gas and hydrogen gas in this experiment? Place your answer for phosphorous gas in the first blank and your answer for hydrogen gas in the second blank.
Hydrogen sulfide (H2S) is a common and troublesome pollutant in industrial wastewaters. One way to remove H2S is to treat the water with chlorine, in which case the following reaction occurs: H2S(aq)+Cl2(aq)→S(s)+2H+(aq)+2Cl−(aq) The rate of this reaction is first order in each reactant. The rate constant for the disappearance of H2SH2S at 28 ∘C is 3.5×10−2 M−1s−1 If at a given time the concentration of H2S is 2.2×10−4M and that of Cl2 is 0.029 M, what is the rate of formation of Cl-? Express the rate in molarity per second to two significant figures.
The rate of formation of Br2 is 6.0 × 10−6 mol/L/s in a reaction described by the following net ionic equation: 5Br− + BrO3 − + 6H+ ⟶ 3Br2 + 3H2 OWrite the equations that relate the rates of consumption of the reactants and the rates of formation of the products.
Consider the reaction, 3NO(g) = N2O(g) + NO2(g). Suppose that at a particular moment during the reaction N2O was being formed at a rate of 3.56 M/h. At what rate is NO reacting? At what rate is the NO2 being formed?
For the decomposition of gaseous dinitrogen pentoxide, 2N₂O₅(g) → 4NO₂(g) + O₂(g) the rate constant is k = 2.8 × 10⁻³ s⁻¹ at 60 °C. The initial concentration of N₂O₅ is 2.95 mol/L in a closed container at 60 °C. After 3.50 min of reaction, what will be the mole fraction of NO₂ in the gaseous mixture? (Don't Hand writing in solution) .
Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of consumption of Br− is 1.16×10−4 M/s over the first two minutes. What is the average rate of formation of H+ during the same time interval?
The rate equation for the reaction A + B = C is rate = k[A][B]. Which of the following is true about the reaction mechanism? The reaction mechanism involves exactly one step. The reaction mechanism involves exactly two steps. The reaction mechanism involves at least two steps. The reaction mechanism involves exactly three steps. The reaction mechanism could involve one, two, three, or more steps.
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.496M 1.63 M 6.00 × 10³ M/s 0.496M 0.191M 82.4M/s 0.209M 1.63 M 2.53 × 10³ M/s Use 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 = k k = | x10 ロ・ロ X
Consider this reaction: →2Cl2O5g+2Cl2g5O2g At a certain temperature it obeys this rate law.rate =0.00711s−1Cl2O5 Suppose a vessel contains Cl2O5 at a concentration of 0.970M . Calculate how long it takes for the concentration of Cl2O5 to decrease to 0.107M . You may assume no other reaction is important.
Consider the reaction : A + 2B → 3C + 4D Suppose that at a particular moment during reaction, C is being formed at the rate of 0.25 Ms-1, at what rate D is being formed in Ms-1? (Do not include the unit of your answer in the answer box and write your answer with 2 significant figures)
Consider the following reaction:2 SO2(g) + O2(g) → 2 SO3 (g)Write the relative rate expressions for all products and reactants in the order they appear in the written reaction. If the rate of consumption of O2 is 0.90 mM/sec at some time in the reaction, what is the rate of formation of the SO3 at the same time in the reaction?
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.496M 1.63 M 6.00 × 10³ M/s 0.496M 0.191M 82.4M/s 0.209M 1.63 M 2.53 × 10³ M/s Use 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 = k k = | x10 ロ・ロ X