Determine the oxidizing agent in this reaction               Sn(s) ∣ Sn2+(aq)  ‖ Ma+(aq) ∣ Ma(s)

For the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?

Assign an oxidation number to the underlined atom in each ion or molecule. (a) Fe2O3, (b) H2SO4, (C) CO32- (C) NO2+

Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).

An electrolytic cell is set up with Cd(s) in Cd(NO3)2(aq) and Zn(s) in Zn(NO3)2(aq). Initially both electrodesweigh 5.00 g. After running the cell for several hours theelectrode in the left compartment weighs 4.75 g. (a) Which electrode is in the left compartment? (b) Does the mass of the electrode in the right compartmentincrease, decrease, or stay the same? If the masschanges, what is the new mass? (c) Does the volume of the electrode in the right compartment increase, decrease, or stay the same? If the volumechanges, what is the new volume? (The density of Cd is8.65 g/cm3.)

From the following list, identify the ions that are more easily reduced than H+(aq). (a) Cu2+(aq) (b) Zn2+(aq) (c) Fe2+(aq) (d) Ag+(aq) (e) Al3+(aq)

Consider these half-reactions: (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Co(s) reduce Pt2+(aq) to Pt(s)? (f) Will Pt(s) reduce Co2+(aq) to Co(s)? (g) Which ions can be reduced by Co(s)?

For the following half-reactions, answer the questions below. Co3+(aq)+eCo2+(aq)E=+1.953VFe3+(aq)+eFe2+(aq)E=+0.769VI2(aq)+2e2I(aq)E=+0.534VPb2+(aq)+2ePb(s)E=0.127VCd2+(aq)+2eCd(s)E=0.402VMn2+(aq)+2eMn(s)E=1.182V (a) Which is the weakest reducing agent? (b) Which is the strongest reducing agent? (c) Which is the strongest oxidizing agent? (d) Which is the weakest oxidizing agent? (e) Will Pb(s) reduce Fe3+(aq) to Fe2+(aq)? (f) Will I-(aq) reduce Pb2+(aq) to Pb(s)? (g) Which ion(s) can be reduced by Pb(s)? (h) Which if any metal(s) can be oxidized by Fe3+(aq)?

Balance each of the following oxidationreduction reactions by using the oxidation states method. a. C2H6(g) + O2(g) CO2(g) + H2O(g) b. Mg(s) + HCl(aq) Mg2+(aq) + Cl(aq) + H2(g) c. Co3+ (aq) + Ni(s) Co2+(aq) + Ni2+(aq) d. Zn(s) + H2SO4(aq) ZnSO4(aq) + H2(g)

What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?