Part AConsider the reaction of ethyl bromide with sodium hydroxide:CH3 CH2B1(aq) + NaOH(aq) = CH3CH2OH(aq) + NaBr(aq)The reaction is first order in NaOH and second order overall. What is the rate law?• View Available Hint(s)O rate = k[CH3 CH,Br] [NaOH]²O rate = k[CH3 CH,Br]NAOH]²O rate = k[N2OH]O rate =k[CH3CH,Br]rate = k(CH3 CH2B1]NAOH]O rate = k(CH3 CH,Br] NaOH]Submit The rate of a chemical reaction depends on theconcentrations of the reactants. Let's consider thegeneral reaction between A and B:aA + bB = cC + dDThe dependence of the reaction rate on theconcentration of each reactant is given by theequation called the rate law.nrate = k[A]" [B]"where k is a proportionality constant called the rateconstant. The exponent m determines the reactionorder with respect to A, and n determines thereaction order with respect to B. The overallreaction order equals the sum of the exponents (m+n).For example, if m = 2 andn=2 thenrate = k[A]2 B]² and the overall reaction order is2+2=4.The reaction orders are experimentally determinedand usually not related to the reactionstoichiometric coefficients a and b.

Consider the reaction of ethyl bromide with sodium hydroxide: CH3 CH2B1(aq)+ NaOH(aq) = CH;CH2OH(aq) + NaBr(aq) The reaction is first order in NaOH and second order overall. What is the rate law? • View Available Hint(s) O rate : k[CH3 CH2 Br] [NaOH O rate= ] k[CH3 CH2 Br|[NaOH rate = k[NaOH] O rate = k[CH3CH,Br] |3D O rate = k(CH3 CH,Br||NaOH O rate = k[CH3CH,Br INAOH] %3D

Consider the reaction of ethyl bromide with sodium hydroxide: CH3 CH2B1(aq)+ NaOH(aq) = CH;CH2OH(aq) + NaBr(aq) The reaction is first order in NaOH and second order overall. What is the rate law? • View Available Hint(s) O rate : k[CH3 CH2 Br] [NaOH O rate= ] k[CH3 CH2 Br|[NaOH rate = k[NaOH] O rate = k[CH3CH,Br] |3D O rate = k(CH3 CH,Br||NaOH O rate = k[CH3CH,Br INAOH] %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

Similar questions

1) Given: 2NO2 --> 2NO + O2 [NO2]o (M) Rate (M/s) 0.01 7.1 x 10-5 0.02 28.1 x 10-5 a) Give the rate law and overall order. b) What is [NO2] at 125 s if [NO2]o = 0.015 M?
What is the rate expression for this reaction?
3 C
Given below is a possible three-step mechanism describing the reaction of hydrogen peroxide with iodide ion in an acidic solution. Step 1: (slow) H2O2(aq) + I-(aq) ---> OH-(aq) + HOI(aq) Step 2: (very fast) OH-(aq) + H+(aq) ---> H2O(liq) Step 3: (fast) HOI(aq) + H+(aq) + I-(aq) ---> I2(aq) + H2O(liq) Assuming that the above reaction mechanism is correct, write the expected rate law expression. Is your experimental data consistent with the proposed mechanism? Explain your answer.
Consider the given reaction in which NC−NC− is the nucleophile and CH3CNCH3CN is the solvent. The reactant molecule has a structure with solid and dashed wedge bonds. A solid wedge () is used to show the bond that is above the plane of the paper, and a dashed wedge () is used to show the bond that is behind the plane of the paper. Draw the product of the following reaction:
Given: 2NO2 --> 2NO + O2 [NO2]o (M) Rate (M/s) 0.01 7.1 x 10-5 0.02 28.1 x 10-5 a) Give the rate law and overall order. b) What is [NO2] at 125 s if [NO2]o = 0.015 M?
The proposed 3-step mechanism for a reaction isStep 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.)Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant) Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] (M) Initial [Y] (M) Initial [Z] (M) Initial Rate (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism.…
Write a balanced reaction for which the following rate relationships are true. Rate (A[NO]/At) = - (1/2)(A[HNO3]/At) = (A[H₂O]/At) = (1/3)(A[NO₂]/At) No +해 + + HNO3 H₂O 1 NO₂ 6 NO3HNO3 6H 20 + 2NO₂ If the rate of disappearance of NO in the reaction in #1 is 0.270 M s-1 at 150°C, the rate of appearance of NO3 is. What is the overall order of the reaction in #1, if given is the rate law? Rate = k[NO]2 [HNO3]³ Ms-1 Given the above rate law, how does the rate of reaction change if the concentration HNO3 is doubled? ANSWER:
Which two the following would be evidence that the mechanism shown below is occurring? When Zno encounters formic acid (HCOOH), the following decomposition reaction occurs. ZnO(aq) + HCООН(9) — Н(g) + CООН() slow step H(g) + COOH(g) CO2(g) + H2(g) + ZnO(aq) fast step HCOOH(g) CO2 + H2(g) overall reaction A The overall reaction is exothermic The addition of the two steps of the В mechanism lead to the overall reaction equation C The overall reaction is endothermic The presence of ZnO(s) increases the rate of the overall reaction E ZnO is an intermediate in the reaction
For each of the following reactions, indicate how the rate of disappearance of each reactant is related to the rate of appearance for each product. 2 H2O2 ---→ 2 H2O + O2 CO + 2 H2 ----> CH3OH B2H6 + 3 O2 ----> B2O3 + 3 H2O
Question is in photo
2