2. Use the table of standard reduction potentials at 25°C, which of these is the most...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Mn + 2 Al3+ → 2 Al + 3 Mn2+ (b) What is n? (c) What is ∆G° for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°?
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Zn + 2 Cr3+ + 2 Cr + 3 Zn? (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°? TABLE 18.1 Standard Reduction Potentials at 25°C EV) 2.87 1.61 1.51 1.36...
(a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: Ca + Sr2+ → Ca2+ + Sr (b) What is the value of E if the concentration of Sr2+ is 8.17 x 10-5 and the concentration of Ca2+ is 8.48 x 10-6? (c) If E = 0.28 V and Sr2+ = 0.10 M, what is the concentration of...
Use the data for the standard reduction potentials in Table 7.1 to predict which of the following is the strongest reducing agent: AgBr, Co2+, H2O, MnO42–
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 2 Nat + Zn → Zn2+ + 2 Na (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°?
consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Al3+(aq) + 3e− → Al(s) − 1.66 Fe2+(aq) + 2e− → Fe(s) − 0.44 Sn2+(aq) + 2e− → Sn(s) − 0.14 The Al/Al3+ half-reaction can be paired with the other two to produce voltaic cells because ________ A) Al is a more powerful oxidizing agent B) Fe and Sn are readily oxidized Al is a more powerful reducing agent C) Al3+ is a more powerful oxidizing agent D) Al3+...
pls explain in great detail why Consider the following standard reduction potentials Reduction Half-Reaction A1+ (aq) + 3e A1(s) Fe2+ (aq) + 2e-Fe(s) Sn2+ (aq) + 2e - Sn(s) E (volts) -1.66 0.44 0.14 The AIAP half-reaction can be paired with the other two to produce voltaic cells because Als* is a more powerful reducing agent OOO Al is a more powerful oxidizing agent o Fe and Sn are readily oxidized Al is a more powerful reducing agent AB+ is...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: Be + 2 Nat → 2 Na + Be2+ (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°? lectrochemical cell described by the followinden and Shaw, and
the standard reduction potential is attached below Use the table of standard reduction potentials for the following exercises. 4. Predict the products of the following redox reactions, then identify which could spontaneously occur. a) H(aq) + Au (s) → b) H (aq) + Na (8) ► c) Au+ (aq) + Na (5) ► 5. Find a reagent that can oxidize Br" to Br2 but cannot oxidize CI'' to Cl? More than one reagent is possible, but you only need to...
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be spontaneous or nonspontaneous in the forward direction in 1.0 Maqueous solution 25°C. a) Snº+(ag) + Ni(s) → Ni2+(aq) + Sna+(aq) b) H2(g) + 2 OH- (aq) + Ca2+(ag) - Ca(s) + 2 H20 (1)