Question 2 of 7SubmitThe oxidation number of oxygen in02- is12346.C78+/-x 10 0Tap here or pull up for additional resourcesN LO

Oxidation number, also called oxidation state . the total number of electrons that an atom either…

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The oxidation number of oxygen in 0²- is

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 65AP

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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)
Which of the following species is being oxidized in this redox reaction? Zn(s)+Cu2+(aq)Zn2+(aq)+Cu(s) a.Zn(s) b.Cu2+(aq) c.Zn2+(aq) d.Cu(s)
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For each of the following balanced half-reactions, determine whether an oxidation or reduction is occurring. (a) Fe3++3eFe (b) CrCr3++3e (c) MnO42MnO4+e (d) Li++eLi
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?
An active (metal) electrode was found to gain mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
Classify the following as acid-base reactions or oxidation-reduction reactions: (a) Na2S(aq)+2HCl(aq)2NaCl(aq)+H2(g) (b) 2Na(s)+2HCl(aq)2NaCl(aq)+H2(g) (c) Mg(s)+Cl2(g)MgCl2(s) (d) MgO(s)+2HCl(aq)MgCl2(aq)+H2+O(l) (e) K3P(s)+2O2(g)K3PO4(s) (f) 2KOH(aq)+H3PO4(aq)K3PO4(aq)+3H2O(l)
In balancing oxidation-reduction reactions, why is it permissible to add water to either side of the equation?
Gold metal will not dissolve in either concentrated nitric acid or concentrated hydrochloric acid It will dissolve, however, in aqua regia, a mixture of the two concentrated acids. The products of the reaction are the AuCl4 ion and gaseous NO. Write a balanced equation for the dissolution of gold in aqua regia.
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?
The Ostwald process for the commercial production of nitric acid involves the following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) 2NO(g)+O2(g)2NO2(g) 3NO2(g)+H2O(l)2HNO3,(aq)+NO(g) a. Which reactions in the Ostwald process are oxidationreduction reactions? b. Identify each oxidizing agent and reducing agent.
2 4 What is the oxidation number of N in N.H₂? Technically if it is positive it should be noted as such but this format will not allow me set +? vs just ?. If it's negative make sure to type in -?