For the reaction2NO + Cl₂Match the appropriate rate law to each postulated mechanism.A Rate = K[NO]²[Cl₂]²B Rate = k[Cl₂]²C Rate =K[NO][Cl₂]D Rate = K[NO]²[Cl₂]Rate =K[NO]²F Rate = k[Cl₂]2NOCINO + Cl₂2NOCI2NOCI 3G Rate =H Rate = K[NO]I None of the aboveK[NO][Cl₂]²NO + Cl₂NOCI₂ + NONOCI₂→→NOCI 3 + NOCI slow→ NOCI + Cl₂ fastCl₂ → 2CICI + NOfast equilibriumNOCI2 fast equilibrium2NOCI slowslowNOCI fast NO + Cl₂2NOCI2NOCI 3NO + Cl₂NOCI₂ + NOCl₂ → 2CICI + NONO + Cl₂NOCI₂ + NONOCI₂ 2NOCI3 + NOCINOCI + Cl₂ fastfast equilibriumslowNOCI₂NOC₂ fast equilibrium2NOCI slowslowNOCI fastNOCI₂ slow2NOCI fastSubmit Answer Tries 0/99

Rate law of reaction is directly proportional to the molar concentration of reactant raised to…

For the reaction 2NO + Cl₂ Match the appropriate rate law to each postulated mechanism. A Rate = K[NO]²[Cl₂]² B Rate = K[Cl₂]² C Rate = K[NO][Cl₂] D Rate = K[NO]²[Cl₂] E Rate = F Rate NO + Cl₂ 2NOCI2 NOCI 3 k[NO]² k[Cl₂] G Rate = K[NO][Cl₂]² H Rate = k[NO] I None of the above NO + Cl₂ NOCI₂ + NO Cl₂ CI + NO 2NOCI 2CI NOCI₂ NOCI 3 + NOCI slow NOCI + Cl₂ fast fast equilibrium NOCI₂ fast equilibrium 2NOCI slow slow NOCI fast

For the reaction 2NO + Cl₂ Match the appropriate rate law to each postulated mechanism. A Rate = K[NO]²[Cl₂]² B Rate = K[Cl₂]² C Rate = K[NO][Cl₂] D Rate = K[NO]²[Cl₂] E Rate = F Rate NO + Cl₂ 2NOCI2 NOCI 3 k[NO]² k[Cl₂] G Rate = K[NO][Cl₂]² H Rate = k[NO] I None of the above NO + Cl₂ NOCI₂ + NO Cl₂ CI + NO 2NOCI 2CI NOCI₂ NOCI 3 + NOCI slow NOCI + Cl₂ fast fast equilibrium NOCI₂ fast equilibrium 2NOCI slow slow NOCI fast

Chemistry

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

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The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2: Step 1: Slow NO2(g) + NO2(g) NO(g) + NO3(g) Step 2: Fast NO3(g) + CO(g) NO2(g) + CO2(g) (a) Show that the elementary steps add up to give the overall, stoichiometric equation. (b) What is the molecularity of each step? (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? (d) Identify any intermediates in tins reaction.
. find the rate law predicted for a particular reaction mechanism.
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
Most reactions occur by a series of steps. The energy profile for a certain reaction that proceeds by a two-step mechanism is On the energy profile, indicate a. the positions of reactants and products. b. the activation energy for the overall reaction. c. E for the reaction. d. Which point on the plot represents the energy of the intermediate in the two-step reaction? e. Which step in the mechanism for this reaction is rate determining, the first or the second step? Explain.
What is the difference between average rate, initial rate, and instantaneous rate?
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.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?

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