for this reaction (including orders). Also give the overall order for this reaction: rate law: overall order = %3D 3. Calculate the rate constant, k, for this reaction (use the data from Experiment #1, show all your work): wollood 4. Explain exactly what experiment(s) must be performed in order to Name Time M T W R F The data given in the table below is for the following reaction (run at 25°C): 2 NOe + O2e) → 2 NO,1e 2(g) 2(g) (g) Initial Concentration (M) Initial rate Experiment Mol/(L s) 02 NO 7 x 10-6 0.0010 0.0010 0.0020 14 x 106 0.0010 0.0030 21 X 10-6 0.0010 0.0030 84 X 106 0.0020 4 189 X 10-6 0.0030 0.0030 2.

for this reaction (including orders). Also give the overall order for this reaction: rate law: overall order = %3D 3. Calculate the rate constant, k, for this reaction (use the data from Experiment #1, show all your work): wollood 4. Explain exactly what experiment(s) must be performed in order to Name Time M T W R F The data given in the table below is for the following reaction (run at 25°C): 2 NOe + O2e) → 2 NO,1e 2(g) 2(g) (g) Initial Concentration (M) Initial rate Experiment Mol/(L s) 02 NO 7 x 10-6 0.0010 0.0010 0.0020 14 x 106 0.0010 0.0030 21 X 10-6 0.0010 0.0030 84 X 106 0.0020 4 189 X 10-6 0.0030 0.0030 2.

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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I just need help with the last 2 questions with correct significant digits
A reaction has two reactants Q and P. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expression? a. rate = k1 b. rate = k2 [P]2 [Q] c. rate = k3 [Q]2 d. rate = k4 [P] [Q] What will the units of the rate constants above be if the rate is expressed in M/min?
3.) The reaction given below is experimentally found to be first order in H2 and third order in NO. SHOW ALL WORK! 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g) a. Write the rate law for the reaction above. b. What is the overall order of the reaction? c. What are the units of the rate constant, k?
25. The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.502 0.502 21600 2 0.502 1.00 43100 3 1.00 0.502 43100 4 1.00 1.00 85800 (a) What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of NO2(g) is 0.505 M and that of O3(g) is 1.37 M if the temperature is the same as that used to obtain the data shown above?______ M/s
d. The mechanism of the reaction is suggested as two steps: NO2+ F2 → NO₂F + F (fast) NO₂+ F→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.
Butadiene reacts to form a dimer according to the equation 2C4H6(g) → C3H₁2(g) The reaction obeys the second order rate law, Rate = K[C4H]², with a rate constant k = 3.68 M-¹min¹ at a certain temperature. Starting with an initial concentration of [C4H6] = 0.0500 M, what will be the butadiene concentration after 43.0 min?
6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2O5). a. Consider this mechanism: i. N2O5 (g) → NO: (g) + NO2 (g) ii. NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (g) i. NO: (g) +0 (g) → NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? [fast) [slow] [fast] b. If the reacuion mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in uNIS nechanism d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.
Consider the rate law. Determine the value of x if the rate doubles when [A] is doubled. X = rate= k[A]* Determine the value of x if no change in rate occurs when [A] is doubled. X = MacBook Pro
The rate of a certain reaction is given by the following rate law: rate -k [N;][H,]* Use this information to answer the questions below. What is the reaction order in Ny? ? What is the reaction order in Hy? 2 What is overall reaction order? At a certain concentration of N, and Hy, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of Ny were doubled? Round your answer to 3 significant digits. M 17.8 The rate of the reaction is measured to be 0.290 M/s when (N)- 1.6 M and [H) - 0.71 M. Calculate the value of the rate constant. Round your answer to 2 significant digits.
2. At low temperatures the rate law for the reaction (½ A+ ½ B → C) is - r₁ =k₁ C₁ CB. If the reaction is reversible at high temperatures, what is the rate law?
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning The reaction C,H, (g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 750.0 K? k = 1.34 x103 Incorrect
I need the last two parts please