Consider the following half-reactions:Half-reactionE° (V)(s) + 2e→ 21°(aq)0.535VNi2*(aq) + 2e→ Ni(s)-0.250VMn2*(aq) + 2e¯→ Mn(s) -1.180V(1) The strongest oxidizing agent is:enter formula(2) The weakest oxidizing agent is:(3) The weakest reducing agent is:(4) The strongest reducing agent is:2+(5) Will I2(s) oxidize Mn(s) to Mn²*(aq)?(6) Which species can be reduced by Ni(s)?If none, leave box blank.

Since you have posted a question with multiple subparts, we will solve the first three subparts for…

Science

Chemistry

L(s) + 2e¯ –→ 21(aq) 0.535 Ni2*(aq) + 2e → Ni(s) |-0.250 Mn2*(aq) + 2e → Mn(s) |-1.180

L(s) + 2e¯ –→ 21(aq) 0.535 Ni2(aq) + 2e → Ni(s) |-0.250 Mn2(aq) + 2e → Mn(s) |-1.180

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

+ 1.14 V TI Pt Cr3+ (1 M) Cr2 (1 M) T13+ (1 M) T13+ (aq) + 3e-→ TI (s) Cr2+ (aq) → Cr3+ (aq) + e- What happens to the thallium electrode as the redox reaction progresses? O it gains mass as thallium metal is plated onto the electrode O it loses mass as the thallium metal is consumed by the reaction O it spontaneously ignites and burns O the thallium electrode is inert and unaffected by the redox reaction O a thick layer of thallium salt develops on the clectrode DELL
Given the reaction: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) Which species is the reducing agent? HCI H2 MgCl2 Mg
Write a balanced redox reaction for the reaction shown below. Cr(s) │ Cr+3 (aq) ║ Fe+2(aq) │ Fe(s)
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 3.255 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0645 M K₂Cr₂O₇ solution required 45.65 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate the mass percent iron in the ore.
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
calculate the standard emf for each of tne following reactions: (a) H2(8) + F(8) → 2H*(aq) + 2 F (aq) (b) Cu2" (aq) + Ca(s) → Cu(s) + Ca²*(aq) (c) 3 Fe2*(aq) → Fe(s) + 2 Fe³*(aq) (d) 2 CIO, (aq) + 10 Br (ag) + 12 H*(aq) → Cl2(8) + 5 Br2(1) + 6 H20(I)
Given the following half-reactions, 2 103 (aq) + 12H*(aq) + 10 e → 12(s) + 6H2O Fe2* (aq) → Fe3* (aq) + e" write the balanced overall reaction. 2103 - (aq) + 12 H* (aq) + Fe 2* (aq) → Fel2 (s) + 6 H2O o 2 103 (aq) + 10 Fe²* (aq) → l2 (s) + 10 Fe³+ (aq) 2 103 - (aq) + 12 H* (aq) + Fe 2* (aq) → 12 (s) + Fe3+ (aq) + 6 H20 2 103 - (aq) + 12 H* (aq) + 10 Fe 2* (aq) → 12 (s) + 10 Fe3+ (aq) + 6 H20
In the following equation Zn(s)+2HCl(aq) → ZnCl2(aq)+H2(g), what is the -species reduced -the reducing agent -the species oxidized -the oxidizing agent
Balance the following oxidation-reduction equation. The reaction occurs in basic solution. Cr20,- (aq)+ S20;²-(aq) → Cr³*(aq) + S,0 (aq)
Balance the following reaction in basic solution. Fill in the coefficients for the balanced overall equation. Al(s) + CrO (ag) → Al(OH)3(s) + Cr(OH), (aq) → 4 4. --v H0+ -- v Al + -v " →-v Al(OH), + -- v Cr(OH), + --v OH CrO, Cr(OH), + -- v OH 4 3.
Balance this equation Mn²+ (aq) +O,(g) Mn0,(s) in basic solution.
Balance the following redox reactions occurring in basic aqueous solution. Identify the species being oxidized, species being reduced, the oxidizing agent, and the reducing agent. ClO- (aq)+Cr(OH)4- > CrO4- + Cl-