Consider these generic half-reactions.Half-reactionOxO y² +● Z³+X+ (aq) + e¯Y2 (aq) + 2 e¯-Z³+(aq) + 3e¯OZ³+O y² +—Identify the strongest oxidizing agent.Z→ X(s)ΟΥX+OZIdentify the strongest reducing agent.Y(s)Z(s)ΟΥOXOx+E° (V)1.490.70-1.22Identify the weakest oxidizing agent.Ox+OzO Y²+O Z³+Identify the weakest reducing agent.X+Z³+YΟΥOxXOzY²+X

We know, Oxidizing agent: oxidize other and undergo reduction itself Reducing agent: Reduce other and undergo oxidation itself So stronger oxidizing agent must have more reduction potential as it has to easily undergo reduction. The stronger reducing agent has lesser reduction potential as it itself likes to undergo oxidation. We can say in this way also Oxidizing agent accepts electron so it is cation An++ne-→A Reducing agent releases electron so it is neutral A→An++ne-Reduction potential- EoX+/X>EoY2+/Y>EoZ3+/z The strongest oxidizing agent X+ as it has highest reduction potential so it can easily get reduced and oxidize other and act as oxidizing agent. The weakest oxidizing agent Z3+ as it has the lowest reduction potential so it hardly undergoes reduction or oxidizes other. The strongest reducing agent Z As, it has more tendency to get oxidize and reduce other. it has less reduction potential. The weakest reducing agent X As, it has less tendency to get oxidize and reduce other. it has large reduction potential.Strongest oxidizing agent X+ Weakest oxidizing agent Z3+ Strongest reducing agent Z Weakest reducing agent X

Science

Chemistry

Consider these generic half-reactions. Half-reaction Ox O y² + Z³+ X+ (aq) + e- Y2 (aq) + 2e Z³+(aq) + 3 e Identify the strongest oxidizing agent. OZ³+ O Y²+ Z Y(s) -Z(s) X(s) ΟΥ X+ Oz Identify the strongest reducing agent. ΟΥ Ox Ox+ E° (V) 1.49 0.70 -1.22 Identify the weakest oxidizing agent. X+ OZ O Y²+ O Z³+ X+ Z³+ Identify the weakest reducing agent. ΟΥ Y X Z y² + X

Consider these generic half-reactions. Half-reaction Ox O y² + Z³+ X+ (aq) + e- Y2 (aq) + 2e Z³+(aq) + 3 e Identify the strongest oxidizing agent. OZ³+ O Y²+ Z Y(s) -Z(s) X(s) ΟΥ X+ Oz Identify the strongest reducing agent. ΟΥ Ox Ox+ E° (V) 1.49 0.70 -1.22 Identify the weakest oxidizing agent. X+ OZ O Y²+ O Z³+ X+ Z³+ Identify the weakest reducing agent. ΟΥ Y X Z y² + X

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

Related questions

Q: Complete and balance the following redox reaction in basic solution Al(s) + OH (aq) → AIO₂ (aq) +…

A: Redox Reaction :Redox reaction is a the reaction that involves the transfer of electrons between…

Q: 11. Balance the following Redox reaction that takes place in basic solution. Identify the oxidizing…

Q: Balance the following redox reaction in acidic solution. O₂(g)+Zn(s) 2+ H₂O(1)+Zn²+ (aq)

A: In the redox reaction, both reduction and oxidation reactions occur simultaneously. One compound is…

Q: The following oxidation-reduction reaction occurs in acidic solution. When the equation is balanced…

Q: In a reactin between copper metal and aqueous iron(III) chloride, Fe3+(aq) is reduced to Fe2+(aq),…

A: The given information says that reaction is a redox reaction. The overall balanced equation for…

Q: Balance the following oxidation-reduction reaction as if it were to occur in a basic solution. I(aq)…

A: The given oxidation-reduction reaction is: I-aq+ClO-aq→I3-aq+Cl-aq

Q: balance the reaction in acidic solution • identify the species oxidized, the species reduced, the…

A: We will give all required information.

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

A: The increase in oxidation no is oxidation & the decrease in oxidation no. Is reduction.

Q: Consider the unbalanced redox reaction shown below: Fe(CN)6-3 (aq) + Re (s) → Fe(CN)6-4…

Q: Balanceando la siguiente reacción redox que ocurre en medio ácido se encuentra que los coeficientes…

A: Redox reaction is combination of reduction and oxidation reaction. In oxidation reaction, oxidation…

Q: Consider the following unbalanced redox reaction. • Part A Cr203 (aq) + Cu (s) → Cr³+(ag) + Cu²+(aq)…

A: In a balanced chemical equation, the atoms of elements on both sides of the equation must be equal.

Q: What element is being reduced in the following redox reaction? C 10H 22O 2( aq) + LiMnO 4( aq) →…

A: ANSWER

Q: Write balanced half-reactions for the following redox reaction: Cr,0; (aq)+7H,0(1)+3 Zn(s) →…

A: To solve this problem we have identifie which species is oxidised and which is reduced .

Q: A(3) NH, + AIO, (aq) O NO, (ag) +H,0() + 2 Al(s) + OH (ag)- NH,)+2 A10, (a O 2 NO, (ag) +H,0(1) + 2…

A: Option A is the right answer.

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

A: Since you have posted multiple question , as per guidelines we can answer one per session . If you…

Q: Calculate the E°cell of the following redox reaction under standard conditions: Zn (s) + MnO ,(s) +…

Q: Which of the following equations represents a spontaneous redox reaction? O O O Zn²+ (aq) (aq) Sn++…

Q: (1). Balance the following redox reaction in a basic solution and indicate which half-reaction is…

A: Given : ClO3-(aq) +Br-(aq)→Cl2(g) +Br2(I)

Q: Write balanced half-reactions for the following redox reaction: 5I2(s)+2Mn2+(aq)+8H2O(l)→…

A: Given : redox reaction

Q: If-reaction identification + e Ag(s) →A*(aq) + 3e" aced equation for the overall redox reaction. Use…

A: Oxidation is loss of Electrons while reduction is Gain of Electrons. Redox REACTION is the reaction…

Q: Balance the following redox reaction equation, which takes place in an acidic solution, using the…

Q: 5. Consider the following half-reactions: F,(g) + 2 e Cu2*(aq) + 2 e Sn2*(aq) + 2 e → AР' (aq) + 3 e…

A: Which of the above elements or ions will oxidize Sn(s)?

Q: Balance the following oxidation-reduction reaction that occurs in an acidic solution using the…

Q: Complete and balance the following redox reaction in acidic solution IO3^-(aq) + ClO2^-(aq) ->…

A: 1 Identify the elements , atoms which undergo oxidation and reduction.2 Balancing charge by cross…

Q: Balance the following redox reaction in acidic solution. H₂O(1) + Cl₂(g) 0₂(g) + Cl (aq) - H₂O (1) +…

Q: Balance the following redox reaction in basic solution. 3+ Cr(OH)3(s) + Fe³+ (aq) 2+ Cro(aq)+ Fe²+…

A: Answer:

Q: Balance the following redox reaction that occurs in acidic conditions: Pt(s) + NO₃⁻(aq) + Cl⁻(aq) ⟶…

Q: Complete and balance the following redox reaction in acidic solution. Be sure to include the proper…

A: Answer:When during a chemical reaction oxidation and reduction take place simultaneously, then such…

Q: 3. In an electrochemical cell oxidation and reduction reactions occurs simultaneously, and it is…

Q: Which of the following is an oxidation-reduction reaction? HCl(aq) + LiOH(aq) → LiCl(aq) + H₂O(l)…

A: Addition of oxygen or removal of hydrogen is oxidation and Addition of hydrogen or removal of oxygen…

Q: Balance the following redox reaction in basic condition. (b) After balancing the equation, indicate…

Q: Balance the following redox reaction in acidic solution using the half reactions method. CuS (s) +…

A: Interpretation- Balance the following given reaction in acidic solution by using half cell reaction…

Q: Balance the following redox reaction in basic solution. Cl(aq)+MnO4(aq) Cl₂(g) + MnO₂ (s)

A: In a redox reaction, both oxidation and reduction reactions occur and it leads to maintaining the…

Q: Write balanced half-reactions for the following redox reaction: 2+ Fe²+ (aq)+NO3(aq) + 2 H+ (aq) 3+…

Q: Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in…

A: Given, MnO 4⁻( aq) + H 2C 2O 4( aq) → Mn 2+( aq) + CO 2( g) The balanced equation in acidic medium…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Consider these generic half-reactions.
Half-reaction
Ox
O y² +
● Z³+
X+ (aq) + e¯
Y2 (aq) + 2 e¯-
Z³+(aq) + 3e¯
OZ³+
O y² +
—
Identify the strongest oxidizing agent.
Z
→ X(s)
ΟΥ
X+
OZ
Identify the strongest reducing agent.
Y(s)
Z(s)
ΟΥ
OX
Ox+
E° (V)
1.49
0.70
-1.22
Identify the weakest oxidizing agent.
Ox+
Oz
O Y²+
O Z³+
Identify the weakest reducing agent.
X+
Z³+
Y
ΟΥ
Ox
X
Oz
Y²+
X

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction
Balance the following redox reaction in the gas phase. Note that this reaction cannot be balanced with the half-reaction method and must be done by inspection. In the gas phase, H2 O (1) is used to balance oxygen atoms and H3 O+ and OH are not available for balancing purposes. ONLY integers should be used in your answer. NH3 (aq) + O2 (g) –→ NO2 (g) Enter your chemical notation here
Write balanced half-reactions for the following redox reaction: H₂ AsO 4(aq) + 8 H* (aq) + 8 Cu* (aq) reduction: oxidation: 2+ AsH₂(g) + 4H₂O(l) +8 Cu²+ (aq)
Write balanced half-reactions for the following redox reaction: 3 Cl,(0)+2 Cr**(aq)+14 OH (aq) → 6 CI (aq)+Cr,0; (aq)+7 H,01) O OP reduction: O-0 oxidation: L
Displacement reaction between copper and zinc. Both metals have an oxidation number of +2 in the cation state. In solution the following reaction can occur. Write the oxidation half-reaction and the reduction half-reaction. Add both half reactions and in the result identify the reducing agent, the oxidizing agent, the oxidized product and the reduced product.
Write balanced half-reactions for the following redox reaction: 51,(s)+2 Mn (aq)+8 H,O(1) 101 (aq)+2 Mno,(aq)+16 H"(aq) reduction: U oxidation: L| e
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
Write balanced half-reactions for the following redox reaction:
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.