Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rateexpression.(a) O + H₂SReactionHO + HS(b) OH + NO2 + N₂ HNO3 + N2(c) CH3CHO → CH3 + CHOMolecularity.][Rate expressionrate =rate =rate =

Answered: Image /qna-images/answer/bf9efe91-2aec-4a4d-99ec-c0c8e1e092ee.jpg

Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction (a) O + H₂S →→→ HO + HS (b) OH + NO2 + N2 (c) CH3CHO HNO3 + N2 CH3 + CHO Molecularity. Rate expression rate = rate = rate =

Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction (a) O + H₂S →→→ HO + HS (b) OH + NO2 + N2 (c) CH3CHO HNO3 + N2 CH3 + CHO Molecularity. Rate expression rate = rate = rate =

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

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
5.) For the reaction X + Y ↓ Z; the reaction rate is found to depend only upon the concentration of X. A plot of 1/[X] verses time gives a straight line. What is the rate law for this reaction?
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
4. The rate law for the reaction H₂ (g) + I₂ (g) → 2 HI (g) was determined to be rate = k [H₂] [1₂], which led to a simple single-step bimolecular mechanism where an H₂ molecule simply collided with an I₂ molecule. In the 1960s, though, different teams found spectroscopic evidence for this mechanism: (1) (2) (3) I₂ (g) →21 (g) H₂(g) + I (g) → H₂I (g) H₂I (g) + I (g) → 2 HI (g) (fast) (fast) (slow) Show that this mechanism is consistent with the rate law: rate = k [H₂] [1₂]. To do this, assign individual rate constants for ALL forward and reverse reactions in the mechanism (I'm guessing k₁, k-1, k2, k-2 and k3). Then show that the overall rate law from combining individual rate laws for the mechanism steps yields rate = (some combination of k's) [H₂] [1₂], and thus k= (some combination of k's). Remember that there should be no reaction intermediates in the rate law, only reactants. \
a) What are the units of the rate constant for a zero-order reaction?b) What are the units of the rate constant if rate =k[A]5[B]3[C]?c) What is the order of reaction for part (b) of this question?
The scenes depict four initial reaction mixtures for thereaction of A (blue) and B (yellow), with and without a solidpresent (gray cubes). The initial rate, -Δ[A]/Δt(in mol/L s),is shown for each sphere representing 0.010 mol and the con-tainer volume at 0.50 L.(a) What is the rate law in the absence of a catalyst?(b) What is the overall reaction order?(c) Find the rate constant.(d) Do the gray cubes have a catalytic effect? Explain.
Please don't provide handwritten solution
2) For each of the following reactions, list three ways in which the rate of the reaction could be increased: i) CaCO3(s) + 2HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l) ii) H₂(g) + 12(g) → 2HI(g) iii) 2H₂O₂(aq) → 2H₂O(1) + O2(g)
Consider the following proposed reaction mechanism: (1) CIO (aq) + H,O(1)= HCIO(aq) + OH (aq) [fast] (2)I (aq) + HCIO(aq) → HIO(aq) + Cl¯(aq) [slow] (3) OH (aq) + HIO(aq) → H,O() + 10 (aq) [fast] Ignoring water, how many reaction intermediates are present? O 3 O 1 O 2
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates.
Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction (a) C₂H5CI → C₂H4 + HCI (b) HO + NO₂ + Ar → HNO3 + Ar (c) O + H₂S →→→→HO + HS Molecularity. Rate expression rate = rate = rate
You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…