The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 → NO₂ + O₂ is first order in NO and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]m [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate= [NO][0₂] -1 S In an experiment to determine the rate law, the rate constant was determined to be 1.15 × 10² M²¹s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 0.182 M and [O3] = 0.0192 M would be 0.402 M/s.

The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 → NO₂ + O₂ is first order in NO and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]m [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate= [NO][0₂] -1 S In an experiment to determine the rate law, the rate constant was determined to be 1.15 × 10² M²¹s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 0.182 M and [O3] = 0.0192 M would be 0.402 M/s.

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 reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 0.0608 M-s¹, when [NO] = 0.498 M and [H₂] = 0.137 M. From this experiment, the rate constant is M-². s-¹.
The gas phase reaction of hydrogen with iodine H₂+I2 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 2.03 x 10-18 M¹s¹. Using this value for the rate constant, the rate of the reaction when [H₂] = 0.0356 M and [1₂] = 0.0123 M would be M/s.
The gas phase reaction of hydrogen with iodine H₂+ 12 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form [A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate In an experiment to determine the rate law, the rate constant was determined to be 2.39 x 10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2]=0.0636 M and [12]=0.0154 M would be M/s. Submit Answer Retry Entire Group more group attempts remaining
The decomposition of nitramide, O₂NNH,, in water has the chemical equation and rate law [O₂NNH₂] [H+] O₂NNH, (aq)- -N₂O(g) + H₂O(1) A proposed mechanism for this reaction is 1.0,NNH, (aq) = O,NNH(aq) + H+ (aq) (fast equilibrium) rate = k 2.0, NNH (aq) N₂O(g) + OH- (aq) (slow) 3. 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? k₂ Answer Bank k_ k3 k
The reaction of nitrogen dioxide with fluorine 2NO2+F2-->2NO2F is first order in NO2 and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n .
The reaction of nitrogen dioxide with carbon monoxideNO2 + CONO + CO2is second order in NO2 and zero order in CO.Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 0.577 Ms-1 when [NO2] = 0.852 M and [CO] = 0.321M. From this experiment, the rate constant i
Q2
The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 7.99 x 10-³ M-s¹, when [NO] = S = 0.192 M and [H₂] = 0.129 M. From this experiment, the rate M².s¹. constant is
The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =
) In studying this reaction, the following mechanism is proposed. k1 A + B C* + B* k2 A + B* C* K3 C* + B D + B* K4 20* → E (product) Find the rate law for the consumption of A. (Assume that k4>>k₁ and k4>>k3).
The gas phase reaction of hydrogen with iodine H₂ + 12 → 2 HI is first order in H₂ and first order in 12. Complete the rate law for this reaction in the box below. Use the form K[A]”[B]". If mor n are 1, don't enter the 1. Omit concentrations taken to the zero power. Rate =