3/28/2017 Homework 5 Bailey Marie Duxworth
CHEM 1202, section 05, Spring 2017
Instructor: John Hogan WebAssign
Homework 5 (Quiz)
Current Score : – / 4 Due : Tuesday, April 18 2017 11:59 PM CDT http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 1/44 3/28/2017 Homework 5 1. –/0.1 pointsBLB11 20.P.019. Complete and balance the following half­reactions. In each case indicate whether the half­reaction is an
oxidation or reduction. (Use the lowest possible coefficients. Include states­of­matter under SATP
conditions in your answer.)
(a) La(s) → La(OH)3(aq) (basic solution) oxidation
reduction (b) TiO2(s) → Ti2+ (acidic solution) oxidation
reduction (c) H2SO3(aq) → SO42­(aq) (acidic solution) oxidation
reduction (d) OH −(aq) → O2(g) oxidation
reduction (e) Sn2+(aq) → Sn4+(aq) oxidation
reduction http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 2/44 3/28/2017 Homework 5 2. –/0.1 points For each of the following reactions, balance the chemical equation, calculate the emf, and calculate G°
at 298 K. (Use the smallest possible coefficients for H2O(l), H+(aq), and HO­(aq). These may be zero.)
(a) Aqueous iodide ion is oxidized to I2(s) by Hg22+(aq). I­(aq) + Hg22+(aq) + H+ I2(s) Hg(l) + H2O(l) emf V G° kJ (b) In acidic solution copper(I) ion is oxidized to copper(II) ion by nitrate ion. Cu+(aq) + + NO3­(aq) + H+(aq) Cu2+(aq) NO(g) H2O(l) emf V G° kJ (c) In basic solution Cr(OH)3(s) is oxidized to CrO42­(aq) by ClO­(aq). Cr(OH)3(s) + (aq) + ClO­(aq) + OH­(aq) CrO42­(aq) Cl­ H2O(l) emf V G° kJ 3. –/0.1 points A voltaic cell is constructed that uses the following reaction and operates at 298 K.
Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ni2+] = 2.81 M and [Zn2+] = 0.180 M? V (c) What is the emf of the cell when [Ni2+] = 0.288 M and [Zn2+] = 0.980 M? V http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 3/44 3/28/2017 Homework 5 4. –/0.1 points A voltaic cell utilizes the following reaction and operates at 298 K.
3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? V (b) What is the emf of this cell when [Ce4+] = 1.3 M, [Ce3+] = 0.013 M, and [Cr3+] = 0.014
M? V (c) What is the emf of the cell when [Ce4+] = 0.54 M, [Ce3+] = 0.88 M, and [Cr3+] = 1.1 M? V http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 4/44 3/28/2017 Homework 5 5. –/0.1 points (a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion. The rate of a fast step has more effect on the overall reaction rate than the rate of a slow step. Solid catalysts do not affect reaction rates. Solid catalysts increase reaction rates as their surface areas increase. The fastest step in a reaction is called the rate­determining step. Reaction rates are determined by reactant concentrations, temperatures, and reactant stabilities. Reaction rates can show little change as masses of solid reactants increase. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 5/44 3/28/2017 Homework 5 6. –/0.1 points A flask is charged with 0.150 mol of A and allowed to react to form B according to the following
hypothetical gas­phase reaction.
A(g) B(g) The following data are collected. times (s)
moles of A 0 40 80 120 160 0.150 0.072 0.049 0.031 0.023 (a) Calculate the number of moles of B at each time in the table. 0 s mol 40 s mol 80 s mol 120 s mol 160 s mol (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. 0 40 s mol/s 40 ­ 80 s mol/s 80 ­ 120 s mol/s http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 6/44 3/28/2017 Homework 5 120 ­ 160 mol/s mol/s http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 7/44 3/28/2017 Homework 5 7. –/0.1 points Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first order in H2(g). What is the rate law
for this reaction? Rate = k [NO(g)] [H2(g)]
Rate = k [NO(g)]2 [H2(g)] Rate = k [NO(g)] [H2(g)]2
Rate = k [NO(g)]2 [H2(g)]2
Rate = k [NO(g)] [H2(g)]3
Rate = k [NO(g)]4 [H2(g)] (b) If the rate constant for this reaction at a certain temperature is 74300, what is the reaction rate
when [NO(g)] = 0.0851 M and [H2(g)] = 0.102 M? Rate = M/s. (c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.170 M while the
concentration of H2(g) is 0.102 M? Rate = M/s http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 8/44 3/28/2017 Homework 5 8. –/0.1 points The reaction 2 ClO2(aq) + 2 OH­(aq) ClO3­(aq) + ClO3­(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH­(aq)] (M) Rate (M/s) 1 0.0494 0.0494 0.0471 2 0.0494 0.0988 0.0943 3 0.0988 0.0494 0.189 4 0.0988 0.0988 0.377 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH­(aq)]
Rate = k [ClO2(aq)]2 [OH­(aq)] Rate = k [ClO2(aq)] [OH­(aq)]2
Rate = k [ClO2(aq)]2 [OH­(aq)]2
Rate = k [ClO2(aq)] [OH­(aq)]3
Rate = k [ClO2(aq)]4 [OH­(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of ClO2(aq) is 0.0929 M and that of OH­
(aq) is 0.101 M if the temperature is the same as that used to obtain the data shown above? http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 9/44 3/28/2017 Homework 5 M/s http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 10/44 3/28/2017 Homework 5 9. –/0.1 points Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the product concentrations rise. As a reaction proceeds forward toward equilibrium the reverse rate constant rises. At equilibrium the rate constants of forward and reverse reactions are equal. At equilibrium all reactions stop. Reactants are transformed into products even at equilibrium. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 11/44 3/28/2017 Homework 5 10.–/0.1 points Gaseous BrCl is placed in a closed container at 995 oC, where it partially decomposes to Br2 and Cl2:
2 BrCl(g) 1 Br2(g) + 1 Cl2(g) At equilibrium it is found that p(BrCl) = 0.002040 atm, p(Br2) = 0.002880 atm, and p(Cl2) = 0.005670
atm. What is the value of KP at this temperature? KP = . 11.–/0.1 points At 301 oC the equilibrium constant for the reaction:
2 HI(g) H2(g) + I2(g) is KP = 2.64e­10. If the initial pressure of HI is 0.00247 atm, what are the equilibrium partial pressures
of HI, H2, and I2? p(HI) = . p(H2) = . p(I2) = . http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 12/44 3/28/2017 Homework 5 12.–/0.1 points Consider the following equilibrium for which H = ­19.51:
2 IBr(g) I2(g) + Br2(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction? (a) Br2(g) is added to the system. ­­­Select­­­ (b) The reaction mixture is cooled. ­­­Select­­­ (c) The volume of the reaction vessel is doubled. ­­­Select­­­ (d) A catalyst is added to the reaction mixture. ­­­Select­­­ (e) The total pressure of the system is increased by adding a noble gas. ­­­Select­­­ (f) I2(g) is removed from the system. ­­­Select­­­ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 13/44 3/28/2017 Homework 5 13.–/0.1 points Choose all of the processes from below which describe changes which are independent of the path by
which the change occurs. the elevation increase experienced by a traveller travelling from Grand Isle, LA to Denver,
Colorado the kinetic energy aquired by a bullet as it reaches a specific speed the work accomplished in burning a gallon of gasoline the latitude increase experienced by a traveller travelling from Baton Rouge, LA to Anchorage,
Alaska the longitude decrease experienced by a traveller travelling from Baton Rouge, LA to London,
England the work generated by a homogeneous gaseous chemical reaction carried out inside of a bomb
calorimeter the enthalpy released by the combustion of a gallon of gasoline http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 14/44 3/28/2017 Homework 5 14.–/0.1 points Consider the following reaction which occurs at constant temperature and pressure:
C6H6(g) 3 C2H2(g) H = 597.2 kJ Which has the higher enthalpy, C6H6(g) or 3 C2H2(g)? C6H6(g)
3 C2H2(g) Without referring to tables indicate which of each of the pairs of choices below has the higher enthalpy: (a)
1 mol of CO2(s) at 50 K
1 mol of CO2(g) at 25 oC (b)
1 mol of He(g) at 300 oC
1 mol of He(g) at 200 oC (c)
1 mol of N2(g) at ­100 oC
1 mol of N2(l) at ­100 oC http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 15/44 3/28/2017 Homework 5 (d)
1 mol of CO2(s) at ­78 oC
1 mol of CO2(g) at ­78 oC http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 16/44 3/28/2017 Homework 5 15.–/0.1 points When a 2.74­g sample of solid sodium nitrate dissolves in 41.5 g of water in a coffee­cup calorimeter
(see above figure) the temperature falls from 22.00 oC to 18.22 oC. Calculate H in kJ/mol NaNO3 for
the solution process.
NaNO3(s) Na+(aq) + NO3­(aq) The specific heat of water is 4.18 J/g­K. Hsolution = kJ/mol NaNO3. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 17/44 3/28/2017 Homework 5 16.–/0.1 points Calculate the standard enthalpy of formation of gaseous hydrogen fluoride (HF) using the following
thermochemical information: C2H4(g) + 6 F2(g) 2 CF4(g) + 4 HF(g) CF4(g) C(s) + 2 F2(g) 2 C(s) + 2 H2(g) H = C2H4(g) H = ­2486.3 kJ
H = +680 kJ
H = +52.3 kJ kJ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 18/44 3/28/2017 Homework 5 17.–/0.1 points The normal condensation point of 1­propanol gas is 97 oC. (a) Is the condensation of 1­propanol gas an endothermic or an exothermic process? This process is an ­­­Select­­­ process. (b) In what temperature range is the condensation of 1­propanol gas a spontaneous process? This process is spontaneous ­­­Select­­­ 97 oC. (c) In what temperature range is this process a nonspontaneous process? This process is nonspontaneous ­­­Select­­­ 97 oC. (d) In what temperature range are the two phases involved in the condensation of 1­propanol gas in
equilibrium? These two phases are in equilibrium ­­­Select­­­ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 97 oC. 19/44 3/28/2017 Homework 5 18.–/0.1 points A certain reaction has Ho = ­80.30 kJ and So = 0.00 J/K. (a) Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is ­­­Select­­­ . (b) Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the
system? This reaction leads to ­­­Select­­­ in the disorder of the system. (c) Calculate Go for this reaction at 298 K. If this value is less than 1 kJ/mol then enter 0 in the answer
box.
Go = kJ. (d) Is this reaction spontaneous, nonspontaneous, or near equilibrium under standard conditions at 298
K? This reaction is ­­­Select­­­ under these conditions. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 20/44 3/28/2017 Homework 5 19.–/0.1 points Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the
following reactions: (a) 3 Fe(s) + 4 CO2(g) Keq = (b) 3 NO(g) Keq = . NO2(g) + N2O(g) . (c) 2 C2H6(g) + O2(g) Keq = Fe3O4(s) + 4 CO(g) 2 C2H4(g) + 2 H2O(g) . http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 21/44 3/28/2017 Homework 5 20.–/0.1 points For each of the following processes, indicate whether the signs of S and H are expected to be
positive, negative, or about zero. (a) Ice cubes melt at 5 oC and 1 atm pressure. For this process S should be ­­­Select­­­ and H should be ­­­Select­­­ . (b) Liquid water is formed from hydrogen and oxygen gases. For this process S should be ­­­Select­­­ and H should be ­­­Select­­­ . and H should be ­­­Select­­­ . (c) A solid sublimes. For this process S should be ­­­Select­­­ (d) Pure solid carbon burns in pure oxygen generating carbon dioxide. For this process S should be Select­­­ and H should be ­­­Select­­­ . (e) A nearly ideal gas is allowed to expand and no temperature change occurs. For this process S should be ­­­Select­­­ and H should be ­­­Select­­­ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 . 22/44 3/28/2017 Homework 5 21.–/0.1 points Complete the following table by calculating the missing entries. In each case indicate whether the
solution is acidic or basic. pH pOH [H+] [OH ­] acidic or
basic?
acidic 13.32 M M basic acidic
1.57 M M basic acidic
5.90 x 10­13 M M basic acidic
M 5.70 x 10­6 M http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 basic 23/44 3/28/2017 Homework 5 22.–/0.1 points Calculate the pH of each of the following strong acid solutions. (a) 0.00108 M HI pH = (b) 0.266 g of HIO4 in 17.0 L of solution pH = (c) 13.0 mL of 4.50 M HI diluted to 4.10 L pH = (d) a mixture formedby adding 38.0 mL of 0.00351 M HI to 79.0 mL of 0.000840 M HIO4 pH = http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 24/44 3/28/2017 Homework 5 23.–/0.1 points Determine the pH of each of the following solutions. (a) 0.495 M boric acid (weak acid with Ka = 5.8e­10). (b) 0.799 M acetic acid (weak acid with Ka = 1.8e­05). (c) 0.230 M pyridine (weak base with Kb = 1.7e­09). http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 25/44 3/28/2017 Homework 5 24.–/0.1 points Calculate the percent ionization of acetic acid (HC2H3O2) in solutions of each of the following
concentrations (Ka = 1.8e­05.) (a) 0.239 M % (b) 0.313 M % (c) 0.769 M % http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 26/44 3/28/2017 Homework 5 25.–/0.1 points (a) Select all of the correct statements about the relative acid strengths of pairs of acids from the
choices below. HCl is a stronger acid than H2S because Cl is more electronegative than S. HAsO42­ is a stronger acid than H2AsO4­ because it has more charge (is more unstable). H3AsO4 is a stronger acid than H2AsO4­ because it has more acidic H atoms. HBrO2 is a stronger acid than HBrO3 because it has fewer oxygens surrounding the central Br
atom. NH3 is a stronger acid than H2O because N is larger than O. HF is a stronger acid than HCl because F is more electronegative than Cl. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 27/44 3/28/2017 Homework 5 26.–/0.1 points (a) Calculate the percent ionization of 0.00430 M hypobromous acid (Ka = 2.5e­09). % ionization = % (b) Calculate the percent ionization of 0.00430 M hypobromous acid in a solution containing 0.0260 M
sodium hypobromite. % ionization = % 27.–/0.1 points A buffer solution contains 0.47 mol of hypochlorous acid (HClO) and 0.90 mol of sodium hypochlorite
(NaOCl) in 3.00 L. The Ka of hypochlorous acid (HClO) is Ka = 3e­08. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.39 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.61 mol of HI? (assume no volume change) pH = http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 28/44 3/28/2017 Homework 5 28.–/0.1 points Consider the titration of 80.0 mL of 0.0200 M NH3 (a weak base; Kb = 1.80e­05) with 0.100 M HIO4.
Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 4.0 mL (d) 12.0 mL pH = pH = (c) 8.0 mL (e) 16.0 mL pH = pH = (f) 25.6 mL http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 pH = 29/44 3/28/2017 Homework 5 29.–/0.1 points (a) If the molar solubility of Cd3(PO4)2 at 25 oC is 1.19e­07 mol/L, what is the Ksp at this temperature?
Ksp = (b) It is found that 0.00100 g of BaCO3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the
solubility­product constant for BaCO3. Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e­31. What is the molar solubility of Sc(OH)3? solubility = mol/L http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 30/44 3/28/2017 Homework 5 30.–/0.1 points A solution of Na2CO3 is added dropwise to a solution that is 0.0725 M in Nd3+ and 3.05e­08 M in Hg22+. The Ksp of Nd2(CO3)3 is 1.08e­33. The Ksp of Hg2CO3 is 3.6e­17. (a) What concentration of CO32­ is necessary to begin precipitation? (Neglect volume changes.) [CO32­] = M. (b) Which cation precipitates first?
Nd3+
Hg22+ (c) What is the concentration of CO32­ when the second cation begins to precipitate? [CO32­] = M. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 31/44 3/28/2017 Homework 5 31.–/0.1 points Choose all of the statements from below which are true about oxidation and reduction. Oxidation and reduction are opposite processes with respect to bookkeeping electrons. Oxidation is what happens when an element in a substance gains electrons. Electrons appear on the right side of an oxidation half reaction. An oxidant is an oxidizing agent, which becomes oxidized during the course of a redox reaction. Reduction is what happens when an element in a substance loses electrons. Electrons appear on the left side of a reduction half reaction. A reductant is an reducing agent, which becomes oxidized during the course of a redox reaction. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 32/44 3/28/2017 Homework 5 32.–/0.1 points Balance the following equations. (Use the lowest possible whole­number coefficients. These may be
zero.) (a) Cr2O72­(aq) + CH3OH(aq) Cr2O72­ + H+ + HCO2H(aq) + Cr3+(aq) CH3OH + H+ + H2O Cr3+ + HCO2H + H2O (b) Cr2O72­(aq) + I­(aq) Cr2O72­ + Cr3+(aq) + IO3­(aq) I­ + H+ + H2O Cr3+ + IO3­ + H+ + H2O (c) ClO­(aq) + Pb(OH)42­(aq) ClO­ + + Pb(OH)42­ + OH­ + H2O Cl­ + PbO2 + OH­ MnO2 + Sn4+ + OH­ H2O (d) MnO4­(aq) + Sn2+(aq) MnO4­ + + Cl­(aq) + PbO2(s) MnO2(s) + Sn4+(aq) Sn2+ + OH­ + H2O H2O http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 33/44 3/28/2017 Homework 5 33.–/0.1 points A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the
top of the figure is a volt meter. One electrode compartment consists of a cobalt strip placed in a 0.5 M
Co2(SO4)3 solution, and the other has a manganese strip placed in a 1.0 M Mn(NO3)2 solution. The
overall cell reaction is: 3 Mn(s) + 2 Co3+(aq) 3 Mn2+(aq) + 2 Co(s) (a) Fill in the information necessary to complete the half reactions that occur in the two electrode
compartments. Use the lowest­possible whole­number coefficients. To input an ion surround the ion's
element symbol with square brackets and put the ion's charge to the right like this: Al3+ = [Al]3+ (not
[Al]+3), and Li+ = [Li]+ (not [Li]1+ or [Li]+1). Do not use brackets for neutral species. Anode half reaction: Cathode half reaction: (s) (aq) + (aq) + e­ e­ (s) (b) Figure out which electrode is the anode, which is the cathode, the signs on these electrodes, the
direction in which the electrons flow through the volt meter, and the direction in which cations and
anions migrate through the salt bridge and solutions. Use this work to pick all of the statements from
below which are true. Electrons flow from the manganese electrode to the cobalt electrode through the volt meter. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 34/44 3/28/2017 Homework 5 The cobalt electrode is the anode and the manganese electrode is the cathode.
Electrons flow from the cobalt electrode to the manganese electrode through the volt meter.
The manganese electrode is the anode and the cobalt electrode is the cathode.
Anions migrate from the 1.0 M Mn(NO3)2 solution through the salt bridge to the 0.5 M Co2(SO4)3
solution.
Cations migrate from the 1.0 M Mn(NO3)2 solution through the salt bridge to the 0.5 M Co2(SO4)3
solution.
Cations migrate from the 0.5 M Co2(SO4)3 solution through the salt bridge to the 1.0 M Mn(NO3)2
solution.
Anions migrate from the 0.5 M Co2(SO4)3 solution through the salt bridge to the 1.0 M Mn(NO3)2
solution.
The manganese electrode is positive and the cobalt electrode is negative.
The cobalt electrode is positive and the manganese electrode is negative. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 35/44 3/28/2017 Homework 5 34.–/0.1 points Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following
reactions if the concentration of each of the ions in these reactions is 0.0009 molar and everything else
is standard (use 298 K for the temperature, R = 8.314 J/mol­K, and F = 96,485 C/mol): (a) 2 Cr3+(aq) + 3 Mn(s) ­­> 2 Cr(s) + 3 Mn2+(aq) E = V (b) 2 Hg2+(aq) + 2 Cu(s) ­­> 1 Hg22+(aq) + 2 Cu+(aq) E = V (c) 2 Na+(aq) + 1 Cu(s) ­­> 2 Na(s) + 1 Cu2+(aq) E = V (d) 2 Cu2+(aq) + 1 Pb(s) ­­> 2 Cu+(aq) + 1 Pb2+(aq) E = V http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 36/44 3/28/2017 Homework 5 35.–/0.1 points Choose all of the statements from below which are true about strengths of oxidants and reductants. The strengths of oxidants and reductants on opposite sides of redox equations correlate
oppositely. For a strong reductant Eored should be positive. Reducing agents are found on the right­hand side of reduction half reactions. For a strong oxidant Eored should be negative. Oxidizing agents are found on the right­hand side of reduction half reactions. http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 37/44 3/28/2017 Homework 5 36.–/0.1 points (a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing
agents in strong acid: Al3+, Ba2+, IO3­, Fe2+, PtCl42­ Al3+ Al3+ Al3+ Al3+ Al3+ Ba2+ Ba2+ Ba2+ Ba2+ Ba2+ IO3­ < IO3­ < IO3­ < IO3­ < IO3­ Fe2+ Fe2+ Fe2+ Fe2+ Fe2+ PtCl42­ PtCl42­ PtCl42­ PtCl42­ PtCl42­ (b) Assuming standard conditions, arrange the following in order of increasing strength as reducing
agents in strong base:
NO, Co2+, Cr, H3AsO3, Br­ NO NO NO NO Co2+ Co2+ Co2+ Co2+ Cr < Cr < Cr < Cr H3AsO3 H3AsO3 H3AsO3 H3AsO3 Br­ Br­ Br­ Br­ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 NO
Co2+ Cr
< H3AsO3
Br­ 38/44 3/28/2017 Homework 5 37.–/0.1 points (a) Choose all of the statements from below which correctly describe issues pertaining to the
relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs.
). Faraday's constant is used to interconvert coulombs of electrons and moles of electrons. Electron stoichiometry need not be used to interconvert a Gibbs free energy change and a reaction
emf. A Gibbs free energy change involves moles of substances whereas an emf involves coulombs of
electrons. Electron stoichiometry must be used to interconvert a Gibbs free energy change and a reaction
emf. Calculate the standard Gibbs free energy changes at 25 oC for each of the reactions shown below using
the Eovalues given. Select whether each of these reactions is nonspontaneous, at equilibrium, or
spontaneous under standard conditions. (a) 1 Cu2+(aq) + 1 Pb(s) 1 Cu(s) + 1 Pb2+(aq) Eo = 0.463 V Go = kJ/mol nonspontaneous
at equilibrium spontaneous (b) 3 Sn4+(aq) + 2 Cr(s) 3 Sn2+(aq) + 2 Cr3+ http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 Eo = 0.894 Go = 39/44 3/28/2017 Homework 5 (aq) V kJ/mol nonspontaneous
at equilibrium spontaneous (c) 1 Mg2+(aq) + 2 Hg(l) 1 Mg(s) + 1 Hg22+ Eo = ­3.159
V (aq) Go = kJ/mol nonspontaneous
at equilibrium spontaneous (d) 1 Cd2+(aq) + 2 Na(s) 1 Cd(s) + 2 Na+(aq) Eo = 2.307 V Go = kJ/mol nonspontaneous
at equilibrium spontaneous http://www.webassign.net/web/Student/Assignment­Responses/last?dep=15136182 40/44 3/28/2017 Homework 5 38.–/0.1 points A electrolytic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following
reaction: 3 Mn2+(aq) + 2 Cr(s) 3 Mn(s) + 2 Cr3+(aq) What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. The positive cell emf rises, becoming more positive.
The positive cell emf drops closer to zero. The negative cell emf rises closer to zero.
The negative cell emf drops, becoming more negative.
No change in cell emf occurs. (b) The size of the manganese electrode is increased. The positive cell emf rises, becoming more positive.
The positive cell emf drops closer to zero. The negative cell emf rises closer to zero.
The negative ce...

 

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