If the reaction X + 2 Y→ XY, occurs by the proposed mechanism, what is the rate 2 law? Step 1 X + Y = XY (slow) Step 2 XY + Y → XY2 (fast) A) rate = k[X] %3D B) rate = k[Y] %3D C) rate = k[Y]? %3D D) rate = k[X][Y] %3D E) rate = k[X][Y]? %3D

If the reaction X + 2 Y→ XY, occurs by the proposed mechanism, what is the rate 2 law? Step 1 X + Y = XY (slow) Step 2 XY + Y → XY2 (fast) A) rate = k[X] %3D B) rate = k[Y] %3D C) rate = k[Y]? %3D D) rate = k[X][Y] %3D E) rate = k[X][Y]? %3D

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

Related questions

Q: The reaction of nitric oxide with hydrogen at 1280°C is 2NO(g) + 2H₂(g) - N₂(g) + 2H₂O(g) From the…

A: Given dataExperiment[NO] (M)[H2] (M)Initial Rate (M/s)15.0 x 10-32.0 x 10-31.3 x 10-5210.0 x 10-32.0…

Q: The complete rate mechanism for a reaction is given below. The rate expression for the rate of the…

A: Suppose a reaction: X + Y ==> Z The rate law is given as : Rate = k [X]m . [Y]n where m+n =…

Q: 12) The data in the table below were obtained for the reaction: A + в — Р Experiment |Initial Rate…

Q: What is the overall reaction order for a chemical reaction with the rate law: rate = k[A][B]? %3D a)…

Q: Consider the following hypothetical chemical reaction A + 2B → E The mechanism for this reaction is:…

A: The correct answer is c) Rate = k[A]2[B] Explanation:Since the rate of a reaction depends on the…

Q: Consider the following data C (aq) + 2 D (aq) - products Experiment Number 1 2 3 [C] 0.020 M 0.030 M…

A: we have to determine the rate law expression for the given reaction

Q: Analyze the following reaction mechanism: 1. H₂O₂ → H₂O + O 2. O + CF₂Cl₂ → CIO + CF₂CI 3. CIO + 03…

A: Answer:Number of species present on the reactant side in a step of a reaction is called as…

Q: A + B à 2C + D , which obeys the rate equation: d[D]/dt k[A]a[B]b [A] (M) [B] (M) d[D]/dt (M/s)…

A: M

Q: What is the correct rate law for the reaction? A) rate = k[NO2]^1[CO]^2 B)rate = k[NO2]^2[CO]^2 C)…

A: According to the rate law, the concentration of reactant species is directly proportional to the…

Q: A reaction, 2NO (g) + O2 (g) 2NO2 (g), was run in a laboratory setting. Given the following…

A: Here we have to determine the rate law and reaction intermediate and if speed of the elementary step…

Q: Consider the following reaction A + 2B + 2C → Products; and its rate formulation: v=k[A][B]² Which…

Q: Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1:…

A: Answer: Rate = k2 [O][N2]

Q: A reaction, 2NO (g) + O2 (g) → 2NO, (g), was run in a laboratory setting. Given the following…

Q: de 12 chemis

A: Chemical kinetics deals with the reaction rates and effects of factors like pressure, temperature,…

Q: Determine the overall order of the following rate laws and the order with respect to each reactant.…

A: Overall reaction order = Sum of the orders with respect to each reactant Orders with respect to…

Q: For the reaction A (g) + B (g) (yields) 2 C (g) The following data were obtained at constant…

A: To solve this problem we have to consider the rate law of given reaction as Rate = K [A]m [B]n…

Q: 7. Substances P and Q react together to form products and the overall order of the reaction is…

A: Rate equation may be defined as an equation that links the rate of forward reaction with the…

Q: How are integrated rate laws used to determine reaction order? What is the order for the reactant…

A: Given Plota) ln [reactant] vs. time is linear? b) 1/[reactant] vs. time is linear? c) [reactant]…

Q: Please don't provide handwriting solutions...

A: The objective of the question is to understand the reaction coordinate diagram for the given…

Q: The following reaction 2 NO(g) + O₂(g) → 2 NO₂(g) was found to be first order in each of the two…

A: In rate equation the sum of the powers of concentration terms indicates the order of the reaction.…

Q: The oxidation of HBr to Br 2 by the reaction 4HB1(g) + O 2(g) 2H 20(g) + 2Br 2(g) is thought to…

A: The overall reaction can be written in steps Step 1 HBr +O2 ----HOOBr Step 2 HOOBr+HBr---2HOBr…

Q: QUESTION 20 The following data was measured for the reaction below. Determine the rate law and the…

Q: Draw different number of X Molecules into three containers using the rate relationships and order…

Q: Consider the reaction below: A → products Using a spectrophotometer, the concentration of A…

A: The given chemical reaction is as follows: A = product For this reaction, a plot of 1/[A] vs. t is a…

Q: 3. Mechanisms and Rate Laws: What is the rate law for the overall reaction based on the proposed…

A: Answer: In the chemical reaction that takes place in more than one step, slowest step of the…

Q: A reaction mechanism has the following proposed elementary steps: Step 1: A B +C Step 2: A + B → D…

A: The rate of reaction is defined as the decrease in the concentration of the reactant or the increase…

Q: The reaction H2(g) + I2(g) → 2HI(g) may occur by the mechanism shown above. What is the rate law…

A: The relation between the concentration of the reactants and the rate of reaction is expressed by the…

Q: What is the rate order with respect to [B] in the reaction A +B → C which has following rate…

Q: What is the overall order for each of the following. a) Rate = k[A]3[B]2b) Rate = k[A]1.5[B]c) A…

A: a) Since the overall order = sum of powers of concentration in the rate equation Since in rate…

Q: 3. Consider the reaction: 1/[HBr] 2 HBr (g) → H₂ (g) + Br₂ (g) Time (s) y = 0.00180 x + .565 a)…

A: Given : Graph and equation Tip : apply second order reaction equation and compare with the given…

Q: What is the rate law for the following reaction and its mechanism? 203-302 (overall reaction)…

A: Explanation to the correct answer is given below

Q: What is the total order for a reaction with rate law r = KIAJ[B]²{C] A) 4 B) 2 O C) 1 D) 3

A: Order of the Reaction is the sum of powers of active concentrations of Reactant Molecules. For the…

Q: Consider the chemical reaction 4 NH3 +702=4 NO2 + 6 H₂O. The differential rate law for this reaction…

A: We have to determine the differential rate law for the given reaction

Question

If the reaction X + 2 Y → XY, occurs by the proposed mechanism, what is the rate
2
law?
Step 1 X + Y= XY (slow)
Step 2 XY + Y → XY2 (fast)
A) rate =
k[X]
B) rate =
k[Y]
C) rate = k[Y]?
D) rate =
k[X][Y]
E) rate = k[X][Y]?

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

A reaction mechanism has the following proposed elementary steps: Step 1: A ⇌ B + C Step 2: A + B → D Step 3: 2 A + D → C + E Which of the following would be the correct elementary rate law for Step 1? A) Rate = k[A] B) Rate = k[A][B] C) Rate = k[A][B][C] D) Rate = k[B][C]
8) Based on the reaction and proposed rate law below, what how should the rate change if the concentration of HBr is tripled and the concentration of O₂ is doubled? 4 HBr + 0₂ → 2 H₂0 +2 Br₂ rate= = k[HBr] A) B) increase by x3 increase by x6 C) D) increase by x 12 increase by x162
Analyze the following reaction mechanism: 1. H₂O2 → H₂O + O 2. O + CF₂Cl2 → CIO + CF₂CI 3. CIO + O3 → CI + 20₂2 4. CI+ CF₂CI → CF₂Cl2 Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF₂CI, CF₂Cl2 C) O, CIO, O, H₂O D) O, CIO, CI, CF₂CI E) O, CIO, CI, CF₂Cl2 ULL
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
Nitrogen(II) oxide, NO, reacts with hydrogen, H2, according to the following equation: 2 NO + 2 H2 - N2 + 2 H20 What would the rate law be if the reaction mechanism occurs in the following steps: Step 1:2 NO + H2 - N2 + H,O2 Step 2: H,02 + H2-2 H20 O rate = k[H2O2]H2] O rate = k[H2O2]|N2] O rate = k[NO]°[H2] O rate = k[H2O]*
Based on the observed rates in the experiments below, what is the rate law for the reaction 3A + 2B + C → G? Expt. # 1 2 3 4 Vo = K[A]²[B][C] Vo = K[A]²[B][C]-1 Vo = K[A]²[B]-¹[C] Vo = K[A][B]²[C] [A] (M) 0.20 0.10 0.10 0.30 [B] (M) 0.10 0.20 0.10 0.10 [C] (M) 0.10 0.20 0.20 0.10 vo (M/s) 0.20 0.050 0.10 0.45
A) In the proposed reaction mechanism below, the intermediate product is: A). NO(g) B). N2O2(g) C). H2(g) D). N2O(g) B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors A) 2 B) 3 C) 6 D) 9
TIA
Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO₂+ Cl₂ → 2NO₂CI (overall reaction) Mechanism NO₂+ Cl2 → NO₂CI+ Cl NO 2 + Cl → NO₂CI A) Rate = k[NO₂] [Cl₂] C) Rate = k[NO₂][CI] = slow fast B) Rate = k[NO₂]²[C]² D) Rate = k[NO₂CI][CI]² E) Rate= k[NO₂CI]
Nitrous oxide, NO, reacts with hydrogen to produce nitrogen and water. The initial rate data obtained for this reaction are given below: NO(g) + H2(g) –→ N2(g) + H2O(l) Using this data, determine the experimental rate law and calculate the rate constant. Experiment [NO] / mol L-1 [H2] / mol L-1 Initial Rate / mol L-1 s-1 1 0.420 0.122 0.136 0.210 0.122 0.0339 3 0.210 0.244 0.0678
. The gas phase reaction X + Y→ Z has a rate law which is experimentally observed to follow the relationship of rate = k[X]2[Y]. If the concentration of X is tripled and the concentration of Y is doubled, the reaction rate would be increased by a factor of: a) 6 b) 9 c) 12 d) 18 e) 36 f) 48 g) 96 h) 128