**Dinitrogen pentoxide decomposes according to the following reaction and rate law:2 N₂O5(g)--> 4 NO2(g) + O₂(g), rate = k [N₂051²The overall reaction order is:E$Ca) 2b) 1c) O4d) 710%FIETTLO5R T406YV BG H4-&799+*UN4+8J$19 144MCKP11OLP77°F a) 2Ob) 1c) 0d) 7e) 5

Chemical kinetics is branch of chemistry in which we deal with the speed at which rate of reaction…

Answered: 205(g)--> 4 NO2(g) + O2(g), rate = k…

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205(g)--> 4 NO2(g) + O2(g), rate = k [N₂O51² overall reaction order is:

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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Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C2(NO2)6, decomposes according to the equation C2(NO2)6- 2NO, + 4NO + 2CO, The reaction in CCl, solvent is first order with respect to Cz{NO2)s At 63.7°C, k= 0.000254 s* and at 112.6°C, k = 0.0126s*. (a) What is the half-life of C2{NO2); at 63.7 °C? i seconds e Textbook and Media (b) What is the half-life of C2(NO2)s at 112.6 °C? seconds (c) IF0.100 mol of C2(NO2)6 is dissolved in CCI4 at 63.7°C to give 1.00 L of solution, what will be the C2(NO2), concentration after 50.0 minutes? i M (d) What is the value of the activation energy of this reaction, expressed in kilojoules? i kJ/mol (e) What is the rate constant at 159.4 °C?
Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO2(g) + O3(g) → NO3(g) + O₂(g) k₁ 2 NO3(g) + NO₂(g) → N₂O5(9) 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: 0 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. rate = k k = 0
Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 hh at 25 ∘C∘C. If a 1.7 −L−L reaction vessel initially contains 760 torrtorr of N2O5N2O5 at 25 ∘C∘C, what partial pressure of O2O2 will be present in the vessel after 230 minutes?
(a) The reaction H2O2(aq)---->H2O(l) + 1/2O2(g) is firstorder. At 300 K the rate constant equals 7.0 x 10-4 s-1.Calculate the half-life at this temperature. (b) If the activationenergy for this reaction is 75 kJ/mol, at what temperaturewould the reaction rate be doubled?
Given the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT). (A) DH = +45 kJ/mol; Ea = 75 kJ/mol; (B) DH = +35 kJ/mol; Ea = 65 kJ/mol; (C) DH = -35 kJ/mol; Ea = 75 kJ/mol; (D) DH = -45 kJ/mol; Ea = 65 kJ/mol;
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s
[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
The rate constant for a first-order reaction is 1.6  10–2s–1at 668 K and 5.1  10–2 s–1at 916 K. What is the activation energy? (R = 8.31 J/(mol · K))
Consider the following balanced chemical equation: H2O2 (aq) + 3 r (aq) + 2 H (aq) >l (aq) + 2 H,O (I) If the concentration of iodide (la) decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s
The rate for the reaction H2 (g) + Br2 (g) 2 HBr (g)is first order in both H2 and Br2 concentrations, and the rate constant k at 287 \deg C is 5.87\times 10-4 L mol-1 s-1. Suppose 1.00 L of H2 (g) at a concentration of 6.60\times 10-2 M is rapidly mixed with the same volume of Br2 (g) also at a concentration of 6.60\times 10-2 M. Calculate the time (in seconds) required for the H2 concentration to decrease to a value of 2.55\times 10-2 M. (Enter your answer to three significant figures.)
Chlorine dioxide, Cl02, is a reddish-yellow gas that is soluble in water. In basic solution it gives Cl03- and CIO2 ions. 2C1O:(aq) + 20н (ад) —> СIО3 (aд) + CIO, (aq) + H;0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Initial Concentration Initial Concentration Initial Rate of Cl02 (mol/L) of OH (mol/L) (mol(L's) Exp. 1 0.21 1.6 x 10-2 0.162 Exp. 2 7.0 x 10-2 1.6 x 10-2 1.80 x 10-2 Exp. 3 7.0 x 10-2 4.8 x 10-2 5.39 х 10-2 a Obtain the rate law. (Use k for the rate constant.) Rate law =
6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?