51 Cr +Balance the equation and determine the reaction. *Cre >24

This is a nuclear reaction and in nuclear reaction there must be mass balance and proton balance.

Answered: Balance the equation and 51 Cr + 24 je…

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Balance the equation and 51 Cr + 24 je > 1 e

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter4: Stoichiometry Of Chemical Reactions

Section: Chapter Questions

Problem 39E: Balance each of the following equations according to the half-reaction method: (a)...

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51 Cr +
Balance the equation and determine the reaction. *
Cr
e >
24

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Similar questions

Balance the following skeleton equations. The reactions occur in acidic or basic aqueous solution, as indicated. a MnO4+S2MnO2+S8(basic) b IO3+HSO3I+SO42(acidic) c Fe(OH)2+CrO42Fe(OH)3+Ce(OH)4(basic) d Cl2Cl+ClO(basic)
Balance each of the following equations according to the half-reaction method: (a) Sn2+(aq)+Cu2+(aq)S4+(aq)+Cu+(aq) (b) H2S(g)+Hg22+(aq)Hg(l)+S(s)(inacid) (c) CN(aq)+ClO2(aq)CNO(aq)+Cl(aq)(inacid) (d) Fe2+(aq)+Ce4+(aq)Fe3+(aq)+Ce3+(aq) (e) HBrO(aq)Br(aq)+O2(g)(inacid)
Balance the following in acidic solution: (a) SO32(aq)+Cu(OH)2(s)SO42(aq)+Cu(OH)(s) (b) O2+Mn(OH)2(s)MnO2(s) (c) NO3(aq)+H2(g)NO(g) (d) Al(s)+CrO42(aq)Al(OH)3(s)+Cr(OH)4(aq)
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
Specify which of the following equations represent oxidation reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced. a. CH4(g)+H2O(g)CO(g)+3H2(g) b. 2AgNO3(aq)+Cu(s)Cu(NO3)2(aq)+2Ag(s) c. Zn(s)+2HCl(aq)ZnCl2(aq)+H2(g) d. 2H+(aq)+2CrO42-(aq)Cr2O72-(aq)+H2O(l)
The blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium di-chromate solution, resulting in the production of Cr3+ (aq) and carbon dioxide. The reaction can be monitored because the dichromate ion (Cr2O72) is orange in solution, and the Cr3+ ion is green. The balanced equations is 16H+(aq) + 2Cr2O72(aq) + C2H5OH(aq) 4Cr4+(aq) + 2CO2(g) + 11H2O(l) This reaction is an oxidationreduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?
In balancing oxidation-reduction equations, why is it permissible to add water to either side of the equation?
Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow. b. Determine the standard cell potential. c. Which electrode increases in mass as the reaction proceeds, and which electrode decreases in mass?

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