A value of k is found from the rate equation Rate = k[A]m[B]". If m=3 and n=3 and the unit for the initial rate is M/h. The unit of k is found to be MX h¯1 (M to the power of x h to the power of minus 1). What is the value of x?

A value of k is found from the rate equation Rate = k[A]m[B]". If m=3 and n=3 and the unit for the initial rate is M/h. The unit of k is found to be MX h¯1 (M to the power of x h to the power of minus 1). What is the value of x?

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 13.4QE

See similar textbooks

Related questions

Q: What are the units of k in the following rate law? Rate = k[X][Y] %3D M3 Ms 一。

A: To solve this problem we will use the given rate law Rate = k[X][Y] .

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

Q: Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following…

A: The balanced reaction taking place is given as, => 2 ClO2 (aq) + 2 OH- (aq) -------> ClO2-…

Q: 3O2(g) →2O3(g) At a given instant, the reaction rate in terms of [O2] is 2.17 ×10−5 mol/L·s. What…

A: Introduction To get the reaction rate in terms of any particular species (either product or…

Q: For a second-order reaction, [A]→products, the rate of the reaction is given as rate= k[A]2, where k…

A: The stimulation for the given reaction is not given. Therefore, the initial concentration [HI]0 and…

Q: Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate…

A: Given: Rate constant = 0.0014 M.s-1 Initial moles of HI = 500.0 mmol Final moles of HI = 250.0 mmol…

Q: Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following…

A: Rate of appearance or the disappearance will be measured by only theoretical way to determine rate…

Q: In the following chemical reaction, if average disappearance rate of B is 0.048 M/sec, then the 2.…

A: In the given chemical reaction, if average disappearance rate of B is 0.048 M/sec, then the…

Q: Find the rate law, including the value of the rate constant k, and fill in the blanks for Exp. 5 and…

A: Answer is explained below. Determination of rate law is as follows:

Q: The rate law for the reaction A + 3B --> C +2D was reported as d[C]/dt=Kr[A][B][C]-1. Express the…

A: The rate law is the chemical expression that tells the relationship between the rate of the reaction…

Q: Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate…

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

Q: A value of k is found from the rate equation Rate = k[A]m[B]n. If m=3 and n=3 and the unit for the…

A: Given: Rate = k[A]m[B]n m=3 and n=3 unit for the initial rate = M/h

Q: Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate…

Q: The reaction for the formation of phosgene from carbon monoxide and chlorine CO + Cl2 COCl2 is…

A: The reaction taking place is given as, => CO + Cl2 -------> COCl2 Given : Reaction is first…

Q: Consider a reaction A + B → C with corresponding rate law rate = k[A]n [B]m If n = 2, m = 1: (a)…

A: Given : Rate law is given as : rate = k[A]n [B]m

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

A: The reaction rates remains unaffected of the species concentrations for the reactions following…

Q: The rate law of a particular reaction is found to be, rate = k[A]²[B]. Which of the following…

A: The rate law for the given reaction is as follows: rate = kA2 B where k = specific rate constant

Q: Consider this reaction: H,CO, (aq) H,0 (aq)+CO, (aq) At a certain temperature it obeys this rate…

A: The rate law of the equation given is, => Rate = 0.067 s-1 [H2CO3] Given: Initial concentration…

Q: Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate…

A: The integrated rate equation for a zero order reaction is k = [R]o - [R] t k = rate constant [Ro] =…

Q: In the following reaction: 2A + B → products, rate = k[A]−1 Determine the rate in terms of the…

Q: Rate = k[X] For the rxn whose rate law is given above, a plot of which of the following is a…

A: Rate = k[X] Order = ?

Q: A certain reaction has the general form cC → dD. At a particular temperature and [C]0 = 2.3 x 10-3…

A: Note: Since we answer up to 3 sub-parts, we'll answer the first 3. Please resubmit the question and…

Q: The rate law for the reaction Cl2 (g) +CHCl3 (g) → HCl (g) +CCl4 (g) is Rate =k[Cl2]1/2 [CHCl3] What…

A: Chemical reaction is given by, Cl2 (g) +CHCl3 (g) → HCl (g) +CCl4 (g) Rate law for the reaction:…

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

Q: The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂ → 2NO₂ is second order in NO and first…

Q: What are the units of the rate constants in the rate law v= kr1[A][B]/(1 + kr2 [B]) when the…

Q: For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C 2 H,O2(aq)2 H,O(1) +…

A: The rate of disappearance of the reactant is the concentration of that reactant decreases in certain…

Q: The reaction of ICl with hydrogen 2 ICI+ H2 –I½ +2 HCl is first order in ICl and third order…

A: According to rate law the rate of reaction depend on concentration of reactant only.

Q: For the reaction X + Y Z, the reaction rate is found to depend only upon the concentration of X. A…

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

Q: According to the differential rate law: rate = k[X]m[Y]n. If m = 2 and n = 1, the overall reaction…

A: • The given rate law equation is, Rate = k[X]m[Y]n where, [X] , [Y] is…

Q: A value of k is found from the rate equation Rate = k[A]M[B]". If m-4 and n-2 and the unit for the…

A: The given data is: m = 4 n = 2 unit for the initial rates = M/h The unit of k found to be Mxh-1.…

Q: 3- A certain reaction has the following general form: At a particular temperature and [A]o = 2.00 ×x…

A: a) Since we know that, for different order of reactions, the relationship between the concentration…

Q: Hydrogen and nitrogen(1I) oxide react according to the following equation. 2H,(g) + 2NO(g) = N,(g) +…

A: for the given reaction, 2H2(g) + 2NO(g) ⇔ N2(g) + 2H2O(g) Rate of the reaction, Rate = k…

Q: Consider the reaction: 2N205(g) → 4NO2(g) + O2(g) At a particular temperature, the rate constant is…

A: Given: Rate constant of the given reaction: 3.81×10-4 s-1. Initial concentration of N2O5 : 0.0212 M.…

Q: Express the rate in terms of change of concentration of A with respect to time where 2A + B ->…

Q: statements are true or false, and explain your answer in one sentence. a) The rate law for an…

A: Order of reaction is an experimental quantity. For elementary reaction, order of reaction is sum…

Q: 4.0 0.0199 M Use this data to answer the following questions. Write the rate law for this reaction.…

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

A: The given reaction is : 2NH3(g) → N2(g) + 3H2(g) Rate constant = 0.0015 M.s-1 Volume of the…

Q: Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of…

A: For zero order reaction: The integrated rate law can be expressed as: [A]o-[A]t = k x t Where, k =…

Q: ) If a reaction has the rate law v = k[A]1[B]0 then what is the power of M that appears in the…

Q: The reaction of nitrogen dioxide with fluorine 2 NO2 + F2 –→ 2 NO2F is first order in NO2 and second…

Q: Consider the hypothetical reaction A +B+ 2C –→ 2D + 3E where the rate law is A[A] k[A][B}* At Rate =…

Q: She fills a reaction vessel with N₂O5 and measures its concentration as the reaction proceeds: time…

A: using the given data we have to calculate rate constant and find rate law expression

Q: Consider a reaction: A + B → C with corresponding rate law: rate = k[A]n [B]m If n = 1, m = 0:…

A: Given n = 1, m = 0:

Q: The reaction 2NO (g) + 02 (g) → 2NO2 (g) has the third-order rate law: rate = k[NO]2 [O2], where k =…

A: Given : Order of reaction = 3 Time = 120 s [NO] = 2.20 x 10-2 M [O2] = 1.10 x 10-2 M K = 25 M-2…

Q: Which of the following is true for the rate law r= k[A]M[B]"? O A) The order of each species must be…

Q: For Rate = k[A]4[B]3, determine the order with respect to reactants and determine the overall…

A: Given data:

Question

A value of k is found from the rate equation Rate = k[A]m[B]". If m=3 and n=3 and
the unit for the initial rate is M/h. The unit of k is found to be MX h¯1 (M to the
power of x h to the power of minus 1). What is the value of x?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

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?
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?
Ozone decomposes to oxygen according to the equation 2O3(g)3O2(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of O3 and the formation of oxygen.
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 4.00 105 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 102 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 102 M C2H5OH to decompose?
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 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.
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?
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)?
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.