d. Determine the rate constant at this temperature 3. In acidsolution, chlorate(V) ions, CIO; slowly oxidize chloride ions to chlorine. Thefollowing kinetic data are obtained at 25 °C.[CH)/ MInitialrate / Ms'10 x 1054.0 x 10[CIO,1/M[H'1/M0.20Experiment0.080.15230.080.150.400.150.308.0 x 1052.0 x 100.160.400.080.20a. Write the halfequation for the oxidation of chloride ion to chlorine.b. Write the balanced equation for this reaction.Given the half equation for reduction is:2CIO, + 10 e + 12H → C, + H20c. Determine the order of the reaction with respect to each rea cta nt.

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3. In acidsolution, chlorate(V) ions, CO, slowly oxidize chloride ions to chlorine. The following kinetic data are obtained at 25 "C. CIO1/M ICH/M 0.15 [H'1/M Initialrate/ Ms' 10x10 4.0 x 10 Experiment 008 0.20 2 0.08 0.15 0.40 3 0.16 0.15 0.40 8.0 x 10 4 0.08 0.30 0.20 20x 104 a. Write the halfequation for the axidation of chloride ion to chlorine. alan

3. In acidsolution, chlorate(V) ions, CO, slowly oxidize chloride ions to chlorine. The following kinetic data are obtained at 25 "C. CIO1/M ICH/M 0.15 [H'1/M Initialrate/ Ms' 10x10 4.0 x 10 Experiment 008 0.20 2 0.08 0.15 0.40 3 0.16 0.15 0.40 8.0 x 10 4 0.08 0.30 0.20 20x 104 a. Write the halfequation for the axidation of chloride ion to chlorine. alan

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 87AP

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Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
4. For the reaction: N20,(9) = 2NO2(g) Assuming initial mass m of N20,(g) and constant temperature (T) and pressure (P). Derive the relation between: (i) The ratio of initial volume V, and average molar mass at equilibrium M2 final volume V, initial molar mass M, (ii) The degree of dissociation a and M, /M2 (Hint: M2 = MN20,Y N20, + M no,Yno2 Y mole fractions ]
Al(OH),(s) = Al³*(aq) +30H¯(aq) X x.- +. log, Cos, K = [AF][OH]; ОН
The below reaction was found to have AH = -406 kJ mol- and AS = 223 J mol-1 K-1. What is AG for this reaction at 118.5 °C? 2Al(s) + 6HCI(aq) – 2AICI;(s) + 3H2(g) Oa. -493 kJ mol-1 Ob. -629 kJ mol-1 Oc. -432 kJ mol-1 Od. -183 kJ mol-1 Oe. -380 kJ mol-1
3. The vapor-liquid reactive equilibria for ethyl lactate synthesis follows the expression log K = 7.893 – (2.4312 x 10³)K/T between 83.12 °C and 101.54 °C. What are the AH°rxn, AG°rxn, and ASºrn at 85 °C? Ind. Eng. Chem. Res. 2008, 47, 5, 1453–1463
An aqueous solution of acetic acid is found to have the following equilibrium concentrations at 25 °C: [CH3COOH] = 1.65 * 10-2 M; [H+]= 5.44 * 10-4 M; and [CH3COO-] = 5.44 * 10-4 M. Calculate the equilibrium constant Kc for the ionization of acetic acid at 25 °C. The reaction is CH3COOH(aq) <=> H+(aq) + CH3COO-(aq)
2. Standar... 1req Consider the reaction: 3. AS surrou 1req 4. AG° =A... 1req 5. AG: Pre... 1req 6. AG: Enthal... M P4010 (8)+6H2O(l) → 4H3PO4(aq) Using standard thermodynamic data at 298 K, calculate the free energy change when 1.80 moles of P4010(s) react at standard conditions. Substance AG (kJ/mol) 7. AG fro... 1req Question Question Question 8. Calculat... 1req 9. Calculat... 1req AG = H3PO4(aq) -1143.0 P4010 (5) -2697.7 H₂O(1) -237.1 kJ 10. Calcul... 1req Submit Answer Retry Entire Group
At a certain temperature, K = 8.30 × 10-4 for the reaction FESCN2+(ag) 2 Fe3+(aq) + SCN¯(aq) Calculate the concentrations of Fe3+, sCN", and FeSCN2+ in a solution that is initially 2.0 M FESCN2+. [FESCN2+] = M [Fe3+] = [SCN"] = M ΣΣ
Calculate the equilibrium constant at 37°C for the reaction Glucose + 60, + 36ADP + 36Phosphaten 6CO, + 42H,0 + 36ATP.. ..... AG° = - 423 kcal/mole ofGlucose
Consider the following equilibrium reaction: Baz(PO4), (s) = 3 Ba2*(aq) + 2 PO,3-(aq) Kc = 3.4 x 10-3 %D 2.00 moles of each reactant and product were placed in 5.00 L of water, mixed and allowed to reach equilibrium. a) Write the Qc expression (LMA) for this reaction. b) Calculate the value of Qc. (Show all work for full credit.) c) In which direction will this reaction proceed to establish equilibrium. Explain your answer. d) Once equilibrium is reached, it was found that the barium ions CHANGED by 0.455 mol. How many moles of each reactant and product are present at equilibrium? (BOX YOUR FINAL ANSWER.)
The equilibrium constant for the reaction H2+122HI Is 20 at 40 °C, and the vapor pressure of solid iodine is 0.1 bar at that temp. If 12.7 g of solid iodine are placed in a 10-dm³ vessel at 40 °C, what is the minimum amount of hydrogen gas that must be introduced in order to remove all the solid iodine?
4A(aq) + 3B(aq) = C(aq) + 8D(ag) AG35SK =? The reaction above was run at 388K and allowed to come to equilibrium. The equilibrium concentrations measured are outlined in the table below: Species Concentration (M) A 8.35 B 7.11 1.49 0.98 Using this information please determine the value AG at this temperature. Please input your answer to the second decimal place in decimal notation. Type your answer.