For the reaction: 2N2O5(g) -->4NO(g) + O2(g) (a) write the mathematical rate expression in terms of (i) the disappearance of N205 (Reactant); (ii) the formation of NO (Product); (iii) the formation of O2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)

For the reaction: 2N2O5(g) -->4NO(g) + O2(g) (a) write the mathematical rate expression in terms of (i) the disappearance of N205 (Reactant); (ii) the formation of NO (Product); (iii) the formation of O2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)

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) 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?
Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?
1. Given the following mechanism for the catalytic destruction of ozone: O3 Оз 02 + 0 O3 + 0 202 (a) Write the overall reaction. (b) What is the intermediate? Explain why. (c) Write all the rate laws for each step (in terms of [O3]). (d) The rate determining step is given as the step 2. Use the steady state approximation to derive the rate law.
The decomposition of B has rate constants of 1.78 x 10-3 min-1 at 25°C and 5.09 x 10-3 min-1 at 45°C. 2 B(aq) -> 3 A(aq) (a) What is the activation energy of the reaction? (b) What is the order of the reaction? (c) How long will it take for a solution containing 0.470 M B to form 0.163 M A at 25°C?
Experiments show that each of the following redox reac-tions is second order overall:Reaction 1: NO₂(g)+CO(g) →NO(g)+CO₂(g) Reaction 2: NO(g)+O₃(g) →NO₂(g)+O₂(g) (a) When [NO₂] in reaction 1 is doubled, the rate quadruples.Write the rate law for this reaction.(b) When [NO] in reaction 2 is doubled, the rate doubles. Writethe rate law for this reaction.(c) In each reaction, the initial concentrations of the reactantsare equal. For each reaction, what is the ratio of the initial rateto the rate when the reaction is 50% complete?(d) In reaction 1, the initial [NO₂] is twice the initial [CO].What is the ratio of the initial rate to the rate at 50% completion?(e) In reaction 2, the initial [NO] is twice the initial [O₃]. Whatis the ratio of the initial rate to the rate at 50% completion?
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
Consider the following reaction: 2A + B + 3C. (a) Write an expression for the overall rate; (b) What are the rates at which A and B are consumed and generated if C is created at a rate of 0.015 M/min?
[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 gas phase reaction between hydrogen and iodine is proposed to occur as follows: step 1: 12 →21 step 2: step 2 H₂ + 2 I (a) Identify the molecularity of each step in the mechanism. step 1 → 2 HI + (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:
The following kinetic data are collected for the initial rates of a reaction 2 X + Z→ products: Experiment [X ]o(M) [Z]o(M) Rate (M/s) 0.25 0.25 4.0 x 10! 0.50 0.50 3.2 x 102 0.50 0.75 7.2 x 102 (a) What is the rate law for this reaction? (b) What is the value of the rate constant with proper units? (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M? 2. 3.
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
Assume that the formation of nitrogen dioxide, 2 NO(g) + 02(g) – 2 NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad О Help Greek - rate=k•[NO]2.[02] rate=k*[NO]^2*[O_2] Correct. (b) A sample of air at a certain temperature is contaminated with 1.9 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. If not, repeat your answer from above. (Rate expressions take the general form: rate = k . [A]ª . [B]b. Use k' for the new rate constant as needed.) chemPad O Help Greek - rate=k':[NO]2 rate=k*[NO]^2 Correct. (c) Under the conditions described in (b), the half-life of the reaction has been estimated to be 6.7x103 min. What would the half-life be if the initial concentration of NO were 12.4 ppm? 4.0 |1030192 X min Supporting Materials Periodic Table Constants and E Supplemental Data