The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate lawO₂NNH, (aq)→ N₂O(g) + H₂O(1)[O₂NNH₂][H+]A proposed mechanism for this reaction is1.0₂NNH₂ (aq) O₂NNH- (aq) + H+ (aq) (fast equilibrium)k-12. O, NNH (aq) N₂O(g) + OH-(aq) (slow)k-rate = k3. H* (aq) + OH(aq) H₂O(l) (fast)What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?k₁k-1Answer Bank

Answered: Image /qna-images/answer/d96ddc49-3821-4b4d-b328-3ec9de2bddfc.jpg

The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH,(aq) N₂O(g) + H₂O(1) [O₂NNH₂] [H+] - A proposed mechanism for this reaction is k₁ 1.0₂NNH, (aq)0₂NNH"(aq) + H* (aq) (fast equilibrium) k= k-1 k₂ rate = k 2. O,NNH (aq) N₂O(g) + OH (aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(1) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k.1 Answer Bank k₂

The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH,(aq) N₂O(g) + H₂O(1) [O₂NNH₂] [H+] - A proposed mechanism for this reaction is k₁ 1.0₂NNH, (aq)0₂NNH"(aq) + H* (aq) (fast equilibrium) k= k-1 k₂ rate = k 2. O,NNH (aq) N₂O(g) + OH (aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(1) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k.1 Answer Bank k₂

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

5. A generic reaction between A and Bas the equation: ZA[aq) + B(s) AzB(aq) To determine the differential rate law, the following experiments were performed with different initial molar concentrations of each: Initial Rate, Experiment [A], M [B), M M/s 1 0.100 0.100 0.00143 2 0.200 0.100 0.00572 3 0.100 0.200 0.00286 a. What is the differential rate law of the reaction? What are the orders b. What is the rate constant with proper units? c. What is the integrated rate law describing the concentration of A at a point in time t for experiment 1? d. How much A is in the reaction solution of experiment 1 at t=2.00 seconds? e. What is the integrated rate law describing the concentration of B at a point in time t for experiment 1? f. How much B is in the reaction solution of experiment 1 at t=2.00 seconds?
The reaction H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature by determining the rate of reaction at reactant concentrations. The results are as follows: N,0 (g) 2. Concentration (M) Rate [NO] (i) (ii) [H] (M/s) 0.25 0.10 0.126 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = k [NO]* [H]°. The exponents x and y represent the order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided.
The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic…
the reaction C4H8(g) --> 2C2H4(g) has an activation energy of 262 kJ/mol. ar 600.0 K the rate constant k is 6.1x10^-8 1/s what is the value of the rate constant at 775.0 K? give answer in standard notation and round to two sig figs
The reaction 2NO(g) + Cl2 (g) -----> 2NOCl (g) was studied at –10°C. The following results were obtained where Rate = - Delta [Cl2]/ delta t [NO]0 [Cl2]0 Initial Rate (mol/L) (mol/L) (mol/L·min) 0.11 0.11 0.24 0.11 0.22 0.48 0.22 0.22 1.92 a Question Content Area What is the rate law? ( Use k for the rate constant. ) Rate =
Based on the initial rates given below, determine the rate constant, k for the following reaction. NH," (aq) + NO2- (aq) → N2 (g) + 2H½O (1I) Rate (Ms-') 2.50 x 10-3 5.00 x 10-3 1.25 x 10-3 Experiment 1 Experiment 2 Experiment 3 NH4" (M) 0.500 NO2 (M) 0.500 0.500 1.000 0.500 0.250 O 0.04 M-1 s-1 0.01 M-1 s-1 0.04 M s-1 O 0.01 M s-1
6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:
Consider the reaction described by the equation C,H,Br, (aq) + 3 I (aq) C,H, (g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k[C,H¸Br,][I¯] where k = 0.00504 M-1. s-1. What are the missing entries in the table? Run [C,H,Br,h (M). [I¯], (M) Initial rate of formation of C,H, (M-s) 1 0.162 0.000529 0.162 y 0.000265 3 0.162 0.162 M X = M y = z = M-s-1
Consider a reaction A → B with activation energy 50.7 kJ/mol. At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature. �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K �K=�∘C+273.15 1 kJ = 1000 J Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!
Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245
Question 17 of 23 Submit Butadiene reacts to form a dimer according to the equation 2C,H6(g) → C3H12(g) The reaction obeys the second order rate law, Rate = k[C,H,]?, with a rate constant k = 3.68 M-'min at a certain temperature. Starting with an initial concentration of [C,H] = 0.0500 M, what will be the butadiene concentration after 31.0 min? | M 1 2 3 C 7 9. +/- x 10 0 LO 00