What is AGⓇ for the following electrochemical equation? (cred (Fe3+/Fe2+) = 0.770 V, cred(Ce++/ Ce3t) =...
Calculate ΔG° for the electrochemical cell Pb(s) | Pb2+(aq) ||
Fe3+(aq) | Fe2+(aq) | Pt(s).A) –1.2 x 102 kJ/molB) –1.7 x 102 kJ/molC) 1.7 x 102 kJ/molD) –8.7 x 101 kJ/molE) –3.2 x 105 kJ/mol
What is ΔG° for the following electrochemical equation? (E°red(K+/K) = –2.931 V, E°red(Ca2+/Ca) = –2.868 V) 2K(s) + Ca2+(aq) → 2K+(aq) + Ca(s) Select one: a. –12 kJ/mol b. –24 kJ/mol c. –6 kJ/mol d. 12 kJ/mol
A student studies the Fe3+/Fe2+ redox pair by using an electrochemical electrode and plotting the electrode potential vs. log10 [Fe3+]/[Fe2+]. Which of the following is correct? A greater ratio of [Fe3+]/[Fe2+] in solution results in Select one: a. a negative gradient b. a lower value of log([Fe3+]/[Fe2+]) c. a higher observed potential A student noticed no change in the potential of a solution of Fe3+/Fe2+ from when the meter was first turned on. Which of the following was most likely...
The following standard reduction potentials have been determined for the aqueous chemistry of iron: Fe3 (a)e>Fe2-(aq 0.770 V Fe2 (aq) 2e>Fe(s E°-0.409 v Calculate the equilibrium constant (K) for the disproportionation of Fe2(aq) at 25 °C. Submit Answer 5 question attempts remaining
+ Given the following electrode potentials at 25°C Fe3+ e-- Fe2+ E° = 0.571 V 2e Fe(s) E° = -0.440 V Calculate the electrode potential for Fe3+ + 3 e- Fe(s) Fe2+ + Select one: a. -0.132 b. -0.036 c. 0.081 d.-0.211 e. 0.103
Use the following standard cell potentials to answer the questions below. Fe3+(aq) + e− ⇌ Fe2+(aq) E° = 0.771 V Ag3+(aq) + e− ⇌ Ag2+(aq) E° = 1.800 V 1. What is ΔG° (in kJ/mol) for this reaction? Report answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol) 2. This reaction is (spontaneous/not spontaneous)
Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) | Fe3+ (aq)| Pt The cell is constructed by preparing one half-cell with a solution containing 8.33 * 10-3 M FeCl3 and 1.67*10-2 M FeCl2, and preparing the other half-cell with a solution containing 8.33*10-3 M CuCl2 and 0.025 M CuCl. Calculate the cell potential once the half-cells are connected to each other. E°(Cu2+/Cu+) = 0.16 V; E°(Fe2+/Fe3+) = 0.77 V
E(Fe3 /Fe2 0.77 V E(Ce ICe -1.70 V 13. In an 8 M HCI and at 45°C medium, titanium (IIl) reduces molybdenum (VI) to molybdenum (V). Draw the i-E curves that correspond to this titration by using a graphite electrode. Data: TI T, fast system with E 0.03 V. Mo /Mo+, slow system with anodic and cathodic potentials of 0.65 and 0.35 V, respectively. E (Cl2/Cr)- 1.4 V 14. Draw the i-E curve for the system: Fe(CN)63, e.-. Fe(CN)64- E"z...
Calculate E°(cell) for the reaction, 2 103"(aq) + 10 Fe2+(aq) <=> 10 Fe3* (aq) + typen the reductor per Fe3+ (aq) + e* <=> Fe2+(aq), E = 0.87 V 2 103(aq) + 10 e<=> 12(aq), E° = 1.10 V A. -7.60 V B. 0.23 V C. -1.97 v D. 1.97 v E. -0.23 V
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...