Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. Use the References to access important values if needed for this question.(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reductionhalf-reaction.half-reactionidentificationCr(s)Cr*("(aq) + 3e"oxidation vF2(g) + 2e-→2F°(aq)reduction(2) Write a balanced equation for the overall redox reaction. Use smallest possible integercoefficients.+

Oxidation is removal of electrons and reduction is addition of electrons.

Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Write a balanced equation for the overall redox reaction. Use smallest possible integer co

Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. Write a balanced equation for the overall redox reaction. Use smallest possible integer co

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter19: Oxidation-reduction(electron Transfer) Reactions

Section: Chapter Questions

Problem 2PE

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Question

Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction.

Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients.

Use the References to access important values if needed for this question.
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction
half-reaction.
half-reaction
identification
Cr(s)Cr*(
"(aq) + 3e"oxidation v
F2(g) + 2e-
→2F°(aq)
reduction
(2) Write a balanced equation for the overall redox reaction. Use smallest possible integer
coefficients.
+

Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.

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Consider three metals, X, Y, and Z, and their salts, XA, YA, and ZA. Three experiments take place with the following results: • X+hotH2Obubbles • X+YAnoreaction • X+ZAXdiscolored+Z Rank metals X, Y, and Z, in order of decreasing strength as reducing agents.
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
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At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
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