The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide:NO₂ + CO → NO + CO₂Experiment [NO₂]0, M1.141.142.292.29123Complete 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'tenter 1 for m or n.Rate = k[NO,] m[CO] Nk =MSubmit Answer1S-1[CO], M Initial Rate, M s•0.1340.7670.2680.7670.1343.090.2683.09-1Retry Entire Group7 more group attempts remaining

The objective of the question is to determine the rate and rate constant.

The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide: NO₂ + CO → NO + CO₂ Experiment [NO2]o, M [CO]o, M Initial Rate, M-s¯¹ 1.14 0.134 0.767 1.14 0.268 0.767 2.29 0.134 3.09 2.29 0.268 3.09 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A]m [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 = k[NO₂][CO] k = M-¹.s-¹ Submit Answer Retry Entire Group 7 more group attempts remaining

The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide: NO₂ + CO → NO + CO₂ Experiment [NO2]o, M [CO]o, M Initial Rate, M-s¯¹ 1.14 0.134 0.767 1.14 0.268 0.767 2.29 0.134 3.09 2.29 0.268 3.09 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A]m [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 = k[NO₂][CO] k = M-¹.s-¹ Submit Answer Retry Entire Group 7 more group attempts remaining

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.49QE: When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay....

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A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.
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Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?