Question

Relative Reduction Potential Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions,...

Relative Reduction Potential Assuming standard conditions, and considering the table of standard reduction potentials for half-reactions, given in your text, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6".

Pb2+ (acidic half-cell solution)
H2O2 (acidic half-cell solution)
Cr3+ (acidic half-cell solution)
Ba
Sn
Al


Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Pb2+ (acidic half-cell solution)

Pb2+ + 2H2O -----> PbO2 + 4H+ + 2e-

Eo = -1.46 V [3]

H2O2 (acidic half-cell solution)

H2O2+2H++2e− --- > 2H2O  

E°= 1.534 V [6]

Cr3+ (acidic half-cell solution)

Cr2O7^2- (aq) +14H+ (aq) + 6 e- --- > 2Cr3+   + 7H2O (l)   E°= +1.33 V [5]


Ba

Ba 2+ (aq)   2e- --- > Ba(s)

E°= -2.90 V [1]

Sn

Sn 2+ (aq)   2e- --- > Sn (s)

E°= - 0.14 V [4]

Al

Al3 + (aq)   3e-    --- > Al (s)

E°= -1.66 V [2]

The compound which have lowest standard reduction potential show strongest reducing property thus here Ba has lowest value thus it is most reducing agent .

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction...
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 480 of Zumdahl 7th ed. yes no  Is H2(g) capable of reducing Ag+(aq)? yes no  Is Fe2+(aq) capable of reducing Cr3+(aq) to Cr metal? yes no  Is Fe2+(aq) capable of oxidizing Cr metal? yes no  Is Fe3+(aq) capable of oxidizing Sn metal to Sn2+(aq)? yes no  Is...
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction...
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed. Is Sn2+(aq) capable of oxidizing Fe2+(aq)? Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)? Is Ni2+(aq) capable of oxidizing H2(g)? Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)? Is Fe2+(aq) capable of oxidizing Cr metal? Is...
Assuming standard conditions, arrange the following in order of decreasing strength as oxidizing agents in acidic...
Assuming standard conditions, arrange the following in order of decreasing strength as oxidizing agents in acidic solution: Cr2O2−7,H2O2,Cu2+,Cl2,O2. I understand that stronger oxidizing agents have more positive cell potentials but how would I figure this out if I weren't given the cell potentials?
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a) O2(g) + Pb(s) → H2O(l) + Pb2+(aq) (b) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq) (c) Cl2(g) + Cr3+(aq) → Cl −(aq) + Cr2O72−(aq) (d) F2(g) + Mn2+(aq) → F −(aq) + MnO4−(aq)
In a table of standard reduction potentials, the strongest oxidizing agents are the _ (blank) _...
In a table of standard reduction potentials, the strongest oxidizing agents are the _ (blank) _ species in the half-reactions with the _ (blank) _ E° values. a. reduced, most negative b. oxidized, most positive c. reduced, most positive d. oxidized, most negative e. none of these
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2...
Short Answer 1) Reduction half-reactions with corresponding standard half-cell potentials are shown below. Zn2+(aq) + 2 e‐ → Zn(s) E° = ‐ 0.76 V Al3+(aq) + 3 e‐ → Al(s) E° = ‐ 1.66 V The standard potential for the galvanic cell that uses these two half-reactions is ________ V. 2)In the galvanic cell represented by the shorthand notation shown below, Cd(aq)|Cd2+(aq)|| I2(g)|I-(aq)|Pt(s) the inert electrode is ________, and the balanced cathode half-reaction reaction is ________.
1. Use a table of Standard Reduction Potentials to predict if a reaction will occur between...
1. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Sn metal and F2(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. 2. Use a table of Standard Reduction Potentials to predict if a reaction will...
Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE...
Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE OXIDIZING AGENT in the final balanced equation: Fe2+ (aq) + MnO4- (aq) ----> Fe3+ (aq) + Mn2+ (aq)      (Acidic Solution)
Using these standard reduction potentials: Reduction Reaction (1) H2O2 + 2e- --> 2OH- E (under std...
Using these standard reduction potentials: Reduction Reaction (1) H2O2 + 2e- --> 2OH- E (under std conditions) (V) = 1.77 (2) [Co(H2O)6]3+ + e- --> [Co(H2O)6]2+    E (under std conditions) (V) = 1.84 (3) [Co(NH3)6]3+ + e- --> [Co(NH3)6]2+ E (under std conditions) (V) = 0.10 Show that one can prepare an ammine complex from CoCl2 and hydrogen peroxide in the presence of ammonia but not in its abscene. You will need to write two redox reactions, calculate standard...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the...
Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT