Help Answering Questions 13

1.

What is the oxidation state of each element in Mn(NO3)2?

N =

2.

Assign oxidation states to the species in the unbalanced redox reaction.

Ag+(aq)+Cu(s)⟶Ag(s)+Cu2+(aq)

Ag+(aq)=

Balance the redox reaction.

redox reaction:

Ag+(aq)+Cu(s)⟶Ag(s)+Cu2+(aq)

3.

The quantity of antimony in an ore can be determined by an oxidation‑reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that all of the antimony is in the form of Sb3+(aq) . The Sb3+(aq) is completely oxidized by an aqueous solution of BrO−3(aq) .

Complete and balance the equation for this reaction in acidic solution.

equation:

BrO−3+Sb3+⟶Br−+Sb5+

4.

Balance the half-reaction in basic solution. Use e− as the symbol for an electron.

half-reaction:

SO2−3⟶S2O2−4

5.

For a particular redox reaction, NO−2 is oxidized to NO−3 and Fe3+ is reduced to Fe2+. Complete and balance the equation for this reaction in basic solution. The phases are optional.

balanced reaction:

NO−2+Fe3+⟶NO−3+Fe2+

6.

Use the activity series interactive to complete the table.

MgZnCuAgMg2+Zn2+Cu2+Ag+

REACTION OR NO REACTION
7.

Consider a galvanic cell in which Al3+ is reduced to elemental aluminum and magnesium metal is oxidized to Mg2+. Write the balanced half-cell reactions that take place at the cathode and at the anode.

half-cell reaction at the cathode:

half-cell reaction at the anode:

8.

Fuel cells are a particular type of electrochemical cell that require a constant source of chemical fuels, or reactants, during operation. One of the most common types of fuel cells is the alkaline fuel cell, which uses hydrogen and oxygen as reactants.

What species are formed at the anode of the alkaline fuel cell?O2H2OH+e−OH−H2What species are formed at the cathode of the alkaline fuel cell?

Write the balanced half‑reaction that occurs at the anode in a hydrogen–oxygen fuel cell in which an alkaline electrolyte is used.

A hydrogen fuel cell. H 2 flows into the cell at the negative electrode. O 2 flows into the cell at the positive electrode. Electrons travel through an external circuit from the negative to the positive electrode. Between the two electrodes is an electrolyte solution. Arrows in the electrolyte point from the positive electrode to the negative electrode.

anode half-reaction:

Write the balanced half‑reaction that occurs at the cathode in a hydrogen–oxygen fuel cell in which an alkaline electrolyte is used.

cathode half-reaction:

Write the balanced overall cell reaction.

overall cell reaction:

H2H2OO2H+OH−e−9.

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