Predict the initial rate of reaction in experiment 4. 13.126. An important reaction in the formation of photochenmic smog is the reaction between ozone and NO: NO(g) + O3(g) → NO2(g) + O,(g) The reaction is first order in NO and O3. The rate constant of the reaction is 80 Ms at 25°C and 3000 M¯' s¯' at 13. 75°C. If this reaction were to occur in a single step, would the rate law be consistent with the observed order of the reaction for NO and O3? h What is the value of the activation energy of the a. reaction? c. What is the rate of the reaction at 25°C when [NO] = 3 X 10-6 M and [O3] = 5 x 10-9 M? %3D %3D d. Predict the values of the rate constant at 10°C and 35°C.

Predict the initial rate of reaction in experiment 4. 13.126. An important reaction in the formation of photochenmic smog is the reaction between ozone and NO: NO(g) + O3(g) → NO2(g) + O,(g) The reaction is first order in NO and O3. The rate constant of the reaction is 80 Ms at 25°C and 3000 M¯' s¯' at 13. 75°C. If this reaction were to occur in a single step, would the rate law be consistent with the observed order of the reaction for NO and O3? h What is the value of the activation energy of the a. reaction? c. What is the rate of the reaction at 25°C when [NO] = 3 X 10-6 M and [O3] = 5 x 10-9 M? %3D %3D d. Predict the values of the rate constant at 10°C and 35°C.

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

The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.80 × 10-4/s at 45°C. If the initial concentration of N2O5 is 7.98×10-2 mol/L, what is the concentration of N2O5 after 503 s? How long would it take for the concentration of N2O5 to decrease to 1.00 × 10-2 mol/L from an initial concentration of 7.98×10-2 mol/L?
Please don't provide handwritten solution ...
john measures the rate constant of a first order reaction to be 1.35 × 102 s-1 at 25.0°C. What is rate constant at 75.0°C if 4.43 × 103 s-1 471 s-1 1.35 × 102 s-1 2.71 × 106 s-1 2.44 × 104 s-1
Dinitrogen pentoxide, N205, decomposes by a first order reaction with an activation energy of 110 kJ/mol. At 65 °C, the rate constant is k = 5.2 x 10-3 s-1. What is the initial rate of reaction when 8.01 g of N,O5 is confined in a 0.75 liter container and heated to 65 °C? A. 3.98 x 10-4 M/s B. 5.14 x 10-4 M/s C. 0.56 x 10-5 M/s D. 2.31 x 10-2 M/s
A reaction of the form aA → Products is second order with a rate constant of 0.711 L/(mol - s). What is the half-life, in seconds, of the reaction if the initial concentration of A is 7.95 x 10- mol L? Half-life =
The dimerization of acetylene: 2C2H2 yields C4H4 is a second order. In one study, at 800 K, it was found that if [C2H2]=.400 M, the reaction occurs at a rate of 2.61 M/min. In another experiment, the reaction proceeds at 800 K with an initial concentration of 0.850M . What will the concentration of acetylene be at t=4.00 min? a) 0.0590 M b) 0.0676 M c)66.7 M d) 0.0150 M e)0.0367 M
The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is: rate = k[A]m[B]n If m is 1, the reaction is first order with respect to A. If the exponent is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If m or n is zero, the reaction is zero order in A or B. If m = 1 and n = 1, the overall order of the reaction is second. (m + n = 1 + 1 = 2). 1. What is the difference between a reaction rate and a reaction's rate constant? 2. What does it mean if a reaction is zero order with respect to a reactant? 3. Doubling the concentration of a reactant increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? 4. Doubling the concentration of a reactant increases the rate of a reaction four times. Tripling the concentration of a different reactant increases the rate of a reaction…
Consider the rate law: Rate = k[NO][O,] Which of the following statements is FALSE regarding this rate law? O The value of k will increase with temperature. O The reaction is 2nd order overall. O The reaction is 1st order with respect to O2 The reaction is 2nd order with respect to NO.
The rate constant for this zero-order reaction is 0.0170 M ·s at 300 °C. A → products How long (in seconds) would it take for the concentration of A to decrease from 0.860 M to 0.320 M? t = S
17
10. For first order reaction A →P with rate constant k = 0.02 s' , how long it would for concentration of A to fall from 0.5M to 0.0005 M? What is half-life of this reaction?
A first-order reaction has a rate constant of 7.5 x 103 s. How many seconds does it take for the reaction to be 39% complete? (Report an integer)