oxygen increases hydrogen lose reducing agent decreases gain oxidizing agent electronsReduction is defined as gain ofDuring reduction, oxidation number of the elementor removal ofand the substance that is reduced acts as a/anor addition offrom a species.Reducing agent is a substance which canelectrons easily.

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oxygen increases hydrogen lose reducing agent decreases gain oxidizing agent electrons or addition of Jor removal of Jand the substance that is reduced acts as a/an Reduction is defined as gain of from a species. During reduction, oxidation number of the element Reducing agent is a substance which can electrons easily.

oxygen increases hydrogen lose reducing agent decreases gain oxidizing agent electrons or addition of Jor removal of Jand the substance that is reduced acts as a/an Reduction is defined as gain of from a species. During reduction, oxidation number of the element Reducing agent is a substance which can electrons easily.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 49QAP

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Similar questions

A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0 ml, of M KMnO4, which oxidizes Fe2+ to Fe3+. The permanganate ion is reduced to manganese(ll) ion. The equation for this reaction is MnO4(aq)+8 H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+ +4H2OAnother 50.00-mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The equation for this reaction is 2Fe3+(aq)+Zn(s)2Fe2+(aq)+Zn2+(aq)The resulting solution is again titrated with 0.0280 M KMnO4; this time 48.0 ml, is required. What are the concentrations of Fe2+ and Fe3+ in the solution?
Which of the following compounds have the same oxidation level, and which have different levels?
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) Al(s)+F2(g) (b) Al(s)+CuBr2(aq) (single displacement) (c) P4(s)+O2(g) (d) Ca(s)+H2O(l) (products are a strong base and a diatomic gas)
Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is NaCl(aq)+H2SO4(aq)+MnO2(s)Na2SO4(aq)+MnCl2(aq)+H2O(l)+Cl2(g) Balance this equation.
Complete and balance the following oxidation-reduction reactions, which give the highest possible oxidation state for the oxidized atoms. (a) K(s)+H2O(l) (b) Ba(s)+HBr(aq) (c) Sn(s)+I2(s)
. For each of the following unbalanced oxidation-reduction chemical equations, balance the equation by inspection, and identify which species is the reducing agent. a.Fe(s)+O2(g)Fe2O3(s)b.Al(s)+Cl2(g)AlCl3(s)c.Mg(s)+P4(s)Mg3P2(s)