34. A key step in the formation of sulfuric acid from dissolvedSO, in acid precipitation is the oxidation of hydrogensulfite ion by hydrogen peroxide:HSO5 (aq) + H2O2 (aq) -The mechanism involves peroxymonosulfurous acid,SO,0OH:HSO, (aq) + H20(e)kiHSO3 (аg) + H02(aq) — SO20OH (аg)+ H:0(€)k-1k2SO20OH¯(aq) + H3O* (aq)→ HSO, (aq) + H3O* (aq)By making a steady-state approximation for the reactiveintermediate concentration, [SO2OOH¯(aq)], express therate of formation of HSO, (aq) in terms of the concentra-tions of HSO3 (aq), H,O2(aq), and H;O*(aq).

Given that, the mechanism of formation of sulfuric acid from the dissolved SO2 in acid precipitation…

34. A key step in the formation of sulfuric acid from dissolved SO, in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO3 (aq) + H2O2(aq) → HSO, (aq) + H2O(e) The mechanism involves peroxymonosulfurous acid, SO,OOH: ki HSO5 (aq) + H2O2(aq) = k-1 SO2OOH¯(aq) + H2O(€) k2 SO20OH (aq) + H:0" (аg) HSO, (aq) + H30* (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO,OOH¯(aq)], express the rate of formation of HSO, (aq) in terms of the concentra- tions of HSO, (aq), H¿O2(aq), and H3O*(aq).

34. A key step in the formation of sulfuric acid from dissolved SO, in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO3 (aq) + H2O2(aq) → HSO, (aq) + H2O(e) The mechanism involves peroxymonosulfurous acid, SO,OOH: ki HSO5 (aq) + H2O2(aq) = k-1 SO2OOH¯(aq) + H2O(€) k2 SO20OH (aq) + H:0" (аg) HSO, (aq) + H30* (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO,OOH¯(aq)], express the rate of formation of HSO, (aq) in terms of the concentra- tions of HSO, (aq), H¿O2(aq), and H3O*(aq).

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

2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?
A reaction profile (not to scale!) for the reaction СНОН + Br—CHBr + OH is shown below: on Е (kJ) C2H5BR + OH 161 71 C2H6ОН + Br Reaction Coordinate Which of the following are true? Choose all that apply. O AE is negative. O The value of Ea in the presence of a catalyst would be lower than 161 kJ. O The value of delta E in the presence of a catalyst would be smaller than 71.0 kJ. O The energy of the products is higher than the energy of the reactants. O The reaction is endothermic.
Reaction CaCO3(s) Ca²+ (aq) + CO3²- (aq) AgCl(s) Ag+ (aq) + Cl(aq) AgBr(s) = Ag*(aq) + Br(aq) Agl(s) Ag+ (aq) + I¯(aq) Initial Concentrations ← [Ca²+] = 1.0 x 10-⁹ M [CO32] = 1.0 x 10⁹ M Ksp = [Ca²+][CO3²-1 X = 3.8 x 10-9 Initial Conditions Q = [1.0 × 10-⁹][1.0 × 10-⁹] = 1.0 x 10-18 Equilibrium Conditions [Ca2+] = 1.0 x 10⁹ M [CO32] 1.0 x 10.⁹ M Mass of CaCO3(s) = 0.0 g 42 of 7 What is the value of the reaction quotient, Q, which is calculated by substituting the actual initial values of [Ca²+] and [CO32] into the equilibrium expression?
Q:4-1 Consider the following reaction: 2 NO(g) + 2 H2(8) → N;(g) + 2 H,O(g) (a) The rate law for this reaction is first order in H, and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 × 10ª M¯²s¯!, what is the re- action rate when [NO] = 0.035 M and [H,] = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H, is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H,] is increased to 0.030 M? %3D Q:4-2 The iodide ion reacts with hypochlorite ion (the ac- tive ingredient in chlorine bleaches) in the following way: OCI- + I- –→ OI¯ + Cl¯. This rapid reaction gives the following rate data: [OCI¯] (M) [I-] (M) Initial Rate (M/s) 1.5 X 10-3 1.5 X 10¬3 1.36 X 10¬4 3.0 × 10–3 1.5 X 10–3 2.72 X 10¬4 1.5 × 10-3 3.0 × 10-3 2.72 X 10¬4 (a) Write the rate law for this reaction. (b) Calculate the rate constant with proper units. (c)…
Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?
A reaction profile (not to scale!) for the reaction 02 + NO2- →03 + NO is shown below: E (kJ) 211 O3 + NO 200 O2 + NO2 Reaction Coordinate Which of the following are true? Choose all that apply. AE is negative. The energy of the products is higher than the energy of the reactants. The reaction is endothermic. The value of Ea in the presence of a catalyst would be lower than 211 kJ. The value of delta E in the presence of a catalyst would be smaller than 200 kJ. Previous
Chlorine dioxide, Cl02, is a reddish-yellow gas that is soluble in water. In basic solution it gives Cl03- and CIO2 ions. 2C1O:(aq) + 20н (ад) —> СIО3 (aд) + CIO, (aq) + H;0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Initial Concentration Initial Concentration Initial Rate of Cl02 (mol/L) of OH (mol/L) (mol(L's) Exp. 1 0.21 1.6 x 10-2 0.162 Exp. 2 7.0 x 10-2 1.6 x 10-2 1.80 x 10-2 Exp. 3 7.0 x 10-2 4.8 x 10-2 5.39 х 10-2 a Obtain the rate law. (Use k for the rate constant.) Rate law =
Construct the expression for Kc for the following reaction. 2 P(s) + 3 Cl(g) 2 PCI (g) Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. [PCL) Ke (PP ICI. Incorrect, 2 attempts remaining Your expression for Kc is incorrect. Recall the general definition of Kc: aA + bB cC + dD Kc = [C]^c [D]^d/ [A]^a [B]^b
Ethyl acetate reacts with sodium hydroxide when the two are mixed. The reaction, called ester hydrolysis, yields products ethyl alcohol and sodium acetate. The equation is CH3CO₂C₂H5(aq) + NaOH(aq) --> C₂H5OH(aq) + CH3CO₂Na(aq) The following data were obtained: Initial Concentration of CH3CO₂C₂Hs (mol L-¹) Initial Concentration of NaOH (mol L-¹) 0.005 0.010 0.005 0.010 0.020 0.020 The rate law for this reaction is: O Rate-k[CH3CO₂C₂H5]²[NaOH] O Rate-k[CH3CO₂C₂H5] + [NaOH] O Rate-k[CH3CO₂C₂H5]²[NaOH)² O Rate-k[CH3CO₂C₂H5] [NaOH] Initial Rate of Formation of C₂H5OH (mol L-1¹) 5.40 x 10-6 2.16 x 10-5 1.08 X 105
Consider the reaction below. What is the effect on the concentration of acetic acid (CH3CO2H), water (H20) hydronium ion (H30*), and acetate ion (CH3CO2) if H3o is added to the reaction? CH3CO2H (aq) + H20 (1) = H30* (aq) + CH3CO2 (aq) Ka=1.8x10-5 The concentration of CH3CO2H The concentration of H30* The concentration of CH3CO2¯ The concentration of H2 increases decreases does not change
1:41 1 .5Gc NH, (aq) B) H+ (aq) + OH¯ (aq) → H₂O (1) C) NH3 (aq) + HI (aq) → NHÂI (aq) D) NH₂ (aq) → NH3 (aq) + H+ (aq) Tap here or pull up for additional resources