16.59 A proposed mechanism for the reaction of carbon dioxide with hydroxide ion in aqueous solution is (1) СО,(ад) + ОН (аq) —> НСО, (аq) (2) HCO,-(aq) + OH¯(aq) → CO,²-(aq) + H,O(1) [fast] [slow] (a) What is the overall equation? (b) Identify the reaction intermediate(s), if any. (c) What are the molecularity and the rate law for each step? (d) Is the mechanism consistent with the actual rate law: k[CO,][OH¯]? rate

16.59 A proposed mechanism for the reaction of carbon dioxide with hydroxide ion in aqueous solution is (1) СО,(ад) + ОН (аq) —> НСО, (аq) (2) HCO,-(aq) + OH¯(aq) → CO,²-(aq) + H,O(1) [fast] [slow] (a) What is the overall equation? (b) Identify the reaction intermediate(s), if any. (c) What are the molecularity and the rate law for each step? (d) Is the mechanism consistent with the actual rate law: k[CO,][OH¯]? 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 decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism: H2O2(aq)+I−(aq)⟶H2O(l)+IO−(aq) (slow) IO-(aq)+H2O2(aq)-->H2O(l)+O2(g) (fast) What is the intermediate, if there is one in the mechanism?
Consider the following proposed reaction mechanism: (1) ClO (aq) + H,O(1) = (2)I (aq) + HCIO(aq) → HIO(aq) + cI (aq) [slow] (3) OH (aq) + HIO(aq) → H,O() + 10 (aq) [fast] HCIO(aq) + OH (aq) [fast] Ignoring the phases of matter, what is the global equation for the mechanism shown here? HCIO + CIO +I + OH → 10' + Cl' + OH " + HCIO O HIO + HCIO + CIO" +I + OH 1O + Cl + OH' + HCIO + HIO + - CIO +l – 10 + Cl O CIO' +I + OH → 10 + Cl' + OH |
For a reaction, A → products, with the rate law: Rate = k[A]2, (a) a plot of ln[A] vs. time gives a straight line. (b) a plot of Rate vs. concentration gives a straight line. (c) both (a) and (b) are correct. (d) a plot of 1/[A] vs. time gives a straight line. (e) both (b) and (d) are correct.
Consider the following balanced chemical equation: H;O2 (aq) + 3 1 (aq) + 2 H* (aq) (aq) + 2 H20 (I) If the concentration of iodide (I3') decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s
Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: step elementary reaction rate constant N,0 (g) → N, (g) +0 (g) k1 1 2 N,0 (g)+0 (g) → N, (g) + 0, (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical ローロ equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k ] Note: your answer should not contain the concentrations of any intermediates. Continue ©2021 McGraw Hill LLC. All Rights
The activation energy of a reaction can be determined from the slope of which of the following graphs? (a) Ink vs. 1 T (b) T 1 VS. In k T (c) In k vs. T In k (d) vs. T T C When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is (a) second (b) more than zero but less than first (c) zero (d) first. 1'5 Loft tion What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C? (R = 8.314 J mol¹ K-¹) (a) 34.7 kJ mol™¹ (c) 342 kJ mol (b) 15.1 kJ mol¹ 1 (d) 269 1-1-t ngha 'kJnz For a reaction between A and B the order with respect to A is 2 and the other with respect to B is 3. The concentrations of both A and B are doubled, the rate will increase by a factor of (a) 12 (c) 32 (b) 16 (K 2 32 A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is (a) 1 (b) 2 (c) 3 da+t In a reaction, A + B → product, rate is doubled when the…
The relative initial rates of the reaction A2 + B2 → products in vessels (a)-(d) are 1:2:4:8. Unshaded spheres represent A2 molecules, and shaded spheres represent B2 molecules present at the beginning of the reaction. 9. 8. o|| 8 (a) (b) (c) (d) What is the order of reaction with respect to A2 What is the order of the reaction with respect to B2 What is the overall order of the reaction?
Chlorine dioxide (CIO,) is a disinfectant used in municipal water- treatment plants. It dissolves in basic solution, producing ClO, and CIO,: 2CIÓ,(g) + 20H'(aq) – CIo,(aq) + CIO,(aq) + H,O(1) Given the data below, what is the order of the reaction with respect to CIO,? Initial [OH] Initial [CIO,] 0.060 Initial Rate (M s1) 0.0248 0.030 0.020 0.030 0.00827 0.020 0.090 0.0247
The reaction 3ClO-(aq) → ClO3-(aq) + 2Cl-(aq) has been proposed to occur by the following mechanism: ClO-(aq) + ClO-( aq)→ ClO2-(aq) + Cl-( aq) (slow) ClO2-(aq) + ClO-(aq) → ClO3-(aq) + Cl-(aq) (fast) Which rate law is consistent with this mechanism? a. rate = k [Cl-][ClO-]2 b. rate = k [ClO-]2 c. rate = k [ClO3-]3 d. rate = k [ClO2-][ClO-] e. rate = k[ClO-]
The relative initial rates of the reaction A 2 + B 2→ products in vessels (a)-(d) are 1:1:4:4. Unshaded spheres represent A 2 molecules, and shaded spheres represent B 2 molecules present at the beginning of the reaction. 8. 8. 8 8|| 8 00 이| 8 6 (a) (b) (c) (d) What is the overall order of reaction? O - N 3
14. The combustion of ethane (C,H,) is represented by the equation: 2C,H.(g) + 70.(g) ) In this reaction: 4CO.(g) +6H,0(I) (a) the rate of consumption of ethane is seven times faster than the rate of consumption of oxygen. (b) the rate of formation of CO, equals the rate of formation of water. (c) water is formed at a rate equal to two-thirds the rate of formation of CO,2. (d) the rate of consumption of oxygen equals the rate of consumption of water. (e) CO, is formed twice as fast as ethane is consumed.
The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism: H2O2(aq)+I−(aq)⟶H2O(l)+IO−(aq) (slow) IO-(aq)+H2O2(aq)-->H2O(l)+O2(g) (fast) What is the chemical equation for the overall process?