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19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following...
Question 10 3.03 pts Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl(s) Ag+ (aq) +CH(aq) Ag+ (aq) +eAg(s) E° =0.7996 VAgCl(s) + e - Ag(s) + CH(aq) E° = 0.22233 V OK-5.2 x 10% spontaneous OK=3.8 x 10nonspontaneous N O K=1.7 x 10-10 nonspontaneous
28. Use the standard reduction potenital to calculate equilibrium constants for the following reaction. H2O (1) H (aq) +OH (aq) at 298.15 K H2 (g)2H (aq) +2e 2H2O (aq) +2e - H2+ 20H (aq) A.K=1.0 x10 B. K=1.6 x10-1l C.K=1.0 x10-14 0 Define electrolvsis. E= 0V E -0.8277 V -10 spontaneous nonspontaneous nonspontaneous
27. Use the standard reduction potenital to calculate equilibrium constants for the following reaction. CdS(s) → Cd2+ (aq) +32 (aq) at 377 K Page 4 of 5 E° = -0.4030 V E° = -1.17 V Cd2+ (aq) +2e → Cd (s) CdS(s) +2e → Ca (s) +S2- (aq) A. K=1.7 x10° nonspontaneous B. K=3.1 x102 nonspontaneous C. K=1.5 x10- nonspontaneous m constants for the fol
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
Calculate the standard Gibbs free energy changes at 25 °C for each of the reactions shown below using the Eº values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 2 Lit(aq) + 2 I'(aq) = 2 Li(s) + 1 12(5) ° = -3.586 V AGC= X kJ/mol nonspontaneous at equilibrium spontaneous (b) 2 CO3+ (aq) + 1 Hg(0) = 2 Co2+ (aq) + 1 Hg2+(aq) ° = 0.988 V AGº =...
Use the data in Appendix L to determine the equilibrium constant for the following reactions. Assume 298.15 K if no temperature is given. (a) AgCl(s) ⇌ Ag+(aq) + Cl−(aq) (b) CdS(s) ⇌ Cd2+(aq) + S2−(aq) at 377 K (c) Hg2+(aq) + 4Br−(aq) ⇌ [HgBr4 ] 2−(aq) (d) H2 O(l) ⇌ H+(aq) + OH−(aq) at 25 °C
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Calculate the value of K given the following information anodel:(oxidation) Fe(s) Fe2+ (aq) + 2e E ? Fe = -0.447 V cathodel:(reduction): 2 x (Ag+ (aq) + e- Ag(s) Eig'lag = 0.7996; V 0.0592 Hint: Use E cell logk Calculate E Cell first. n 2.6 O 1.247 O 1.3X1042 none of the above
Using the following standard reduction potentials Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions. Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s) Group of answer choices E° = -0.90 V, spontaneous E° = -0.90 V, nonspontaneous E° = +0.90 V, nonspontaneous E° = +0.90...
Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77 V Pb2+ (aq) + 2 e. → Pb(s) E。--0.13 V Calculate the standard cell potential for the galvanie cell reaction given below, and determine whether or not this reaction is spostaneous under standard conditions. Pb2+ (aq) + 2 Fe2+ (aq) → 2 Fe3+ (aq) + Pb(s) ⓔ A. E.-0.90 V, nonspontaneous OB. E-0.90 V, spontaneous C. Eo +0.90 V, nonspontaneous OD0.90 V, spontaneous