The cell potential E for the cell Pt(s) | H2(g, =1.00) | H(aq, =1.00) | NaCl(aq, 0.300 m) | AgCl(s) | Ag(s) at 25°C is +0.260 V. Determine the mean activity coefficient Y+.
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- For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)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.
- From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)Electrochemical cell Pt | H2(g) | Hl(aq) || Ag|(s) | Ag(s)has electromotive potential of 0.52 V at 25°C. Find the pH.
- The cell potential E for the cell Pt(s) H2(g, =1.00) H (aq, =1.00)| NaCI(aq, 0.100 m) AgC(s) Ag(s) at 25°C is +0.280 V. Determine the mean activity coefficient y.Consider the cell: Pt(s) | H₂(g, 0.100 bar) | H+ (aq, pH = 2.54) || Cl(aq, 0.200 M) | Hg₂Cl₂(s) | Hg(1) | Pt(s) Use the following information to calculate the cell potential. Hg₂²+ (aq) + 2e- → 2Hg(1) 2H+ (aq) + 2e- → H₂(g) Hg₂Cl₂(s) → Hg₂²+(aq) + 2Cl¯(aq) E° = 0.796 V E° = 0.000 V Ksp = 1.2 X 10-18Consider the cell: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) | Hg() | Pt(s) Use the following information to calculate the cell potential. Hg2Cl2(s) + 2e− ® 2Hg() + 2Cl−(aq) E ° = 0.268 V 2H+(aq) + 2e− ® H2(g) E ° = 0.000 V
- Determine the emf for the cell Ag (s) | AgCl (s) | HCl (a = 1) | Cl2 (1 atm) | Pt given that the standard electrode potential of the Ag (s) | AgCl (s) | Cl- (aq) electrode is 0.2225 V, and that of the Pt | Cl2 (g) | Cl- (aq) is 1.3595 V.[1.137] The answer is written in the bracket. I would like to know how it is obtained. Thank you!The standard potential of the cell Bi(s)|Bi2S3(s)|Bi2S3(aq)|Bi(s) is +0.96 V at 25 °C. Calculate the equilibrium constant for the dissolution of Bi2S3(s).Determine the reaction and the emf for the cellZn | Zn2+ (a = 0.1) || Cl- (a = 0.2), Hg2Cl2 (s) | Hg (l) if the standard electrode potential of the Zn | Zn2+ (aq) electrode is − 0.763 V, and that of the Hg | Hg2Cl2 (s) | Cl- (aq) is 0.268 V.[1.031] The answer is written in the bracket. Thank you!