3. Look up the standard reduction potentials (E°) for the Au³⁺/Au and Ni²⁺/Ni couples (Resource Section 3 in your book) and use them to determine the direction of the unbalanced reaction (acidic solution) shown below.\[ \text{Au(s) + Ni}^{2+}\text{(aq)} \leftrightarrow \text{Au}^{3+}\text{(aq) + Ni(s)} \](a) Write the fully balanced reaction (be sure to clearly indicate in which direction the reaction will proceed).(b) Calculate the E° value for the reaction in part a.(c) Identify the oxidizing agent, the reducing agent, which species gets oxidized, and which species gets reduced.

3) a) in balanced chemical reaction number of atoms of each element in product side is equal to…

*(aq) → Au²*(aq) + Ni(s) ne fully balanced reaction (be sure to clearly indicate in which direction th a will proceed). te the E° value for the reaction in part a. the oxidizing agent, the reducing agent, which species gets oxidized, and gets reduced.

(aq) → Au²(aq) + Ni(s) ne fully balanced reaction (be sure to clearly indicate in which direction th a will proceed). te the E° value for the reaction in part a. the oxidizing agent, the reducing agent, which species gets oxidized, and gets reduced.

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 reaction shown, which occurs in aqueous solutions: NO2^-1 + Al (s) --> NH3 + Al(OH)4^-1 Identify the species reduced: Identify the species oxidized: Identify the reducing agent: Identify the oxidizing agent: The balanced reduction half-reaction: The balanced oxidation half-reaction: Overall balanced redox reaction:
Using standard reduction potentials from the ALEKS Deta tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. Cu (aq) + HNO₂ (aq) + H* (aq) → Cu² (aq) + NO(g) + H₂O (1) X
Formation of iodine from iodide. Assign oxidation numbers to each atom. Identify the oxidizing agent and the reducing agent. 211-(aq) + Mn02(s) + 4 H+ (aq) → I2(s) + Mn²+(aq) + 2 H20(1)
2Ag + HPO,²+ H,0→H¿PO,¯ + Ag,0+ OH¯ 2-+ In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent:
A. Balance the following redox reactions using the half-reaction method. B. Identify the oxidizing agent and the reducing agent. 1. Zn(s) + Fe²+ (aq) → Zn²+ (aq) + Fe (s) 2+ Zn(s) → Zn² +2e- oxidiation haut reaction (aq) 2+ 20+ Fe (an) → Fe (5) Reducation haut reaction (94) - Bris) Reducing agent (S) Fe 2+ oxidizing agent 2. (Balance this reaction In Acidic Solution):
Chati kar bhainn steps show karing q6 6. Balance the following redox reaction in acid solution: SO2 (g) + Cr2O7^-2(aq) SO4^-2(aq) + Cr3+ (aq)
Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cl2 and OH- in the balanced reaction?Cl2(g) → ClO3-(aq) + Cl-(aq)
Write balanced half-reactions for the following redox reaction: 1₂(s)+2 NO₂(g) + 2 H₂O(1) → 21 (aq) + 2NO3(aq) + 4H* (aq) reduction: oxidation: 0 ロ→ロ X
Classify each half-reaction as a reduction or an oxidation. 10⁰00 Cr₂O² (aq) + 14 H+ (aq) + 6 e¯ → 2 Cr³ ¹(aq) + 7 H₂O(1) Fe³+ (aq) + 3 e - Fe(s) Au(s) + 2 CN (aq) - → Au(CN)₂ (aq) + e¯ HgO(s) + H₂O(1) + 2 e¯ → Hg(1) + 2 OH (aq) 2 CI (aq) → Cl₂(g) + 2 e Answer Bank oxidation reduction
Identify the weakest oxidizing agent and weakest reducing agent given the following. A) CГ (ag), Ba*" (aq) Half reaction E° red Cl2 (g) + 2e¯→ 2CI¯ (aq) В) Ва** (аq), СГ (aq) +1.35827 Br2 (aq) + 2e-→ 2B1¯ (aq) +1.0873 C) Ba (s), Cl2 (g) I2 (S) + 2e→ 21 (aq) +0.5355 Zn2* (aq) + 2e→ Zn (S) D) Cl2 (g), Вa (s) -0.7618 2+ Ва (ад) + 2е — Ва (s) -2.912 E) CI2 (g), Ba? (аq)
The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.