10 QuestionSee page 837The axidation of NH4 to NO3 in acid solution (pH = 5.600) is described by the following equation:NH(ag) + 20,(e) → No, (ag) + 2H* (aq) + H,0(1)The overall reaction for the oxidation has an Ecen-0.2710 V.E°- 1.50 V for the half-reactionNO, (ag) + 10H"(ag) + 8e" NH{(aq) + 3H,0(1)See Periodic Table O See HintBe sure to solve the equation using a base-10 logarithm (log) rather than the natural logarithm (In).What is the ratio of [NO, ] to [NH4'lat 298 Kif Poz- 0.180 atm? Assume that the reaction is at equilibrium.

Given:- The pH of the solution is 5.60 Eocell=-0.2710 V Eo for half reaction =-1.50V. Find:= The…

he oxidation of NH, to NO3 in acid solution (pH = 5.600) is described by the following equation: NH|(a9) + 20,(2) → NO; (ap) + 2" (ap) + H,0() The overall reaction for the oxidation has an E'cer -0.2710 V. E- 1.50V for the half-reaction NO, (ag) + 10H"(ag) + 8e NH(aq) + 3H,0() d See Periodic Table O See Be sure to solve the equation using a base-10 logarithm (log) rather than the natural logarithm (In). What is the ratio of (NO,I to [NH'lat 298 Kif Po2-0.180 atm? Assume that the reaction is at equilibrium.

he oxidation of NH, to NO3 in acid solution (pH = 5.600) is described by the following equation: NH|(a9) + 20,(2) → NO; (ap) + 2" (ap) + H,0() The overall reaction for the oxidation has an E'cer -0.2710 V. E- 1.50V for the half-reaction NO, (ag) + 10H"(ag) + 8e NH(aq) + 3H,0() d See Periodic Table O See Be sure to solve the equation using a base-10 logarithm (log) rather than the natural logarithm (In). What is the ratio of (NO,I to [NH'lat 298 Kif Po2-0.180 atm? Assume that the reaction is at equilibrium.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e Cu2+ → Hg(1) 0.855V *(aq) + 2e¯ → Cu(s) 0.337V Fe2+(aq) + 2e" - Fe(s) -0.440v| (1) The strongest oxidizing agent is: enter for ula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Fe2+(aq) oxidize Hg(1) to Hg2+(aq)? (6) Which species can be oxidized by Cu2+(aq)? If none, leave box blank.
4) For the following reactions, (i) write the half-reactions, (ii) write a balanced equation for the whole reaction, (iii) determine in which direction the reaction will proceed spontaneously under standard state conditions: H2(g) + Ni2+(aq) ---------> Ni(s) + H+(aq) Cr3+ + Zn(s) ----------> Cr(s) + Zn2+(aq)
9. Write a Nernst expression, at 25 °C, for the following half-reactions: (a) Zn* (aq) + 2 e- 5 Zn (s) (b) Fe* (aq) + e- s Fe2* (aq) (c) 2 H* (aq) + 2 e- H2 (g) (d) Cr2O2- (aq) + 6 e + 14 H* (aq) S 2 Cr* (aq) + 7 H2O (I)
Chegg.... Grades f... Grades f... 0 O ELECTROCHEMISTRY Using the Nernst equation to calculate nonstandard cell voltage Workshe... A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) + 5 Co²+ (aq) x10 Suppose the cell is prepared with 4.59 MIO3 and 4.70 M H in one half-cell and 7.33 M Co 2+ Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0.0 X A ALEKS -... μ 00 www-awy.aleks.com M Sign In I... 5 2. h Hulu | Pr... in the other. Home
Give a clear handwritten answer with explanation
Please answer fast I'll rate you sure
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…
Balance the following reaction in basic solution. Ag(s) + Zn²+(aq) → Ag,O(ag) + Zn(s) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. -- v Ag + -- v Zn2+ + v Zn + Ag,0 + -- v--