1. Balance each equation. Use the oxidation number method for a), c), and e). Use the half reaction method for b), d), and f). a) Sn + NO3 → H₂SnO3 + NO (acidic conditions) Ox #method b) Cr₂0,2+ Fe 2+ Cr 3+ + Fe3+ (acidic Conditions) 1/2 rxn

Consider the following half-reactions: Explain why platinum metal will dissolve in aqua regia (a mixture of hydrochloric and nitric acids) but not in either concentrated nitric or concentrated hydrochloric acid individually.

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)

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?

. 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)

Chromium has been investigated as a coating for steel cans. The thickness of the chromium film is determined by dissolving a sample of a can in acid and oxidizing the resulting Cr3+ to Cr2O72 with the peroxydisulfate ion: S2O82(aq) + Cr3+(aq) + H2O(l) Cr2O72(aq) + SO42(aq) + H+(aq) (Unbalanced) After removal of unreacted S2O82 an excess of ferrous ammonium sulfate [Fe(NH4)2(SO4)26H2O] is added, reacting with Cr2O72 produced from the first reaction. The unreacted Fe2+ from the excess ferrous ammonium sulfate is titrated with a separate K2Cr2O7 solution. The reaction is: H+(aq) + Fe2+(aq) + Cr2O72(aq) Fe3+(aq) + Cr3+(aq) + H2O(l) (Unbalanced) a. Write balanced chemical equations for the two reactions. b. In one analysis, a 40.0-cm2 sample of a chromium-plated can was treated according to this procedure. After dissolution and removal of excess S2O82, 3.000 g of Fe(NH4)2(SO4)26H2O was added. It took 8.58 mL of 0.0520 M K2Cr2O7 solution to completely react with the excess Fe2+. Calculate the thickness of the chromium film on the can. (The density of chromium is 7.19 g/cm3)

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)

Which of the following compounds have the same oxidation level, and which have different levels?

Determine the oxidation number of each element in each of the following compounds: (a) HCN (b) OF2 (c) ASCl3

In balancing oxidation-reduction equations, why is it permissible to add water to either side of the equation?