HomeworkLib
Question

Please answer all parts to this question! parts a through e! This is all one question so I could not post them separately, please also check your answers because the last person got it wrong! Thank you! Will give thumbs up. a. Which of the following species will be reduced by Zn(s), but not by Ag(s) under standard conditions? O Pb(s) O Mg2+(s) O Cc. Which of the following is the strongest oxidizing agent? O Pb2+ (aq) O 12(s) O Ag+ (aq) Pb(s) O Cu2+ (aq) O Br (aq) Q5.4 1Q5.5 1.8 Points e. In the galvanic cell described in the multiple choice question immediately above, what happens to the cell

engineering   Chemical-Engineering   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Answers: (a) None of the above

(b) Pb(s)

As Pb is present in between above Ag and below Zn in the activity series , it has higher tendency to get oxidised than Ag but lesser tendency to get oxidised than zinc. Hence, Ag+ can get reduced to Ag and oxidise Pb to Pb2+.

(c) Ag+

(d) Pb(s) ----> Pb2+(aq) + 2e-

As lead is above silver in the activity series, the reduction potential of lead will be less than silver. So, silver will be placed in cathode and get reduced while lead will be in anode and get oxidised.

(e) It remains the same

Since Ag is in solid state, its volume is negligible and hence is neglected in calculating reaction quotient for determining cell potential. Hence, cell potential remains same.

0 0
Add a comment
Know the answer?
Add Answer to:
Please answer all parts to this question! parts a through e! This is all one question...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • this is all part of the same question! will give thumbs up! thanks! a. Which of...

    this is all part of the same question! will give thumbs up! thanks! a. Which of the following species will be reduced by Zn(s), but not by Ag(s) under standard conditions? O Pb(s) O Mg2+ (8) O Cl2(9) Au(s) O A13+ (aq) O None of the above Q5.2 1.8 Points b. Which of the following species will be oxidized by Ag+ (aq), but not by Zn2+ (aq) under standard conditions? O Pb(s) O Mg2+ (s) O Cl2(9) O Au(s) O...

  • both of these are part of the same question so I could not post them separately!...

    both of these are part of the same question so I could not post them separately! please answer both its the same question! will give thumbs up d. Consider a galvanic cell consisting of a Pb2+/Pb half cell and a Ag+ /Ag half cell. Assuming standard conditions, which of the following represents the reaction that occurs at the anode of this cell? O Pb2+ (aq) + 2e + Pb(s) O Pb(s) + Pb2+ (aq) + 2e O Ag+ (aq) +...

  • can you answer questions 7,8,9,10 Question 7 (10 points) ✓ Saved (7) For a galvanic cell...

    can you answer questions 7,8,9,10 Question 7 (10 points) ✓ Saved (7) For a galvanic cell notation: (-) Mg/Mg2+ (aq) // Cu2+ (aq) / Cu (+). which of the following is fully correct? (a) Mg2+ is oxidized to Mg, and Cu2+ (aq) is reduced to Cu O (b) Mg2+ is reduced to Mg, and Cu2+ (aq) is oxidized to Cu (c) Mg is oxidized to Mg2+, and Cu²+ (aq) is reduced to Cu (d) Mg is reduced to Mg2+, and...

  • For each set of materials below: i.Write the cell notation (line notation)for a galvanic cell and...

    For each set of materials below: i.Write the cell notation (line notation)for a galvanic cell and ii.Calculate the standard cell potential a. Pb(s), Zn(s), Pb2+(aq),Zn2+(aq) b. Ag(s), Fe(s), Ag+(aq),Fe2+(aq) c. Mg(s), Zn(s), Mg2+(aq),Zn2+(aq) d. Fe(s), Mg(s), Fe2+(aq), Mg2+(aq e. Ag(s), Pb(s), Pb2+(aq), Ag+(aq) 2. For each set of materials below: Write the cell notation (line notation) for a galvanic cell and Calculate the standard cell potential ii. a. Pb (). Zn (3), Pb2+(aq), Zn2+ (aq) 6. Ag (3), Fe (3),...

  • can you please help.me answer these three questions please? I am really desperate and in need...

    can you please help.me answer these three questions please? I am really desperate and in need of help. Question 10 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and Al3+ (aq)/Al(s) electrodes. Ni2+(aq) + 2e - Ni(s) Ered = -0.257 V Al3+(aq) + 3e Al(s) Eºred = -1.676 V Calculate AG° 0 -273.9 kJ ho O-821.6 kJ 0 -410.8 kJ +821.6 kJ O +273.9 kJ Question 11 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and...

  • Hi. can some one please explain me the solution for this question. the correct answer is...

    Hi. can some one please explain me the solution for this question. the correct answer is C. thanks. 8. Consider the following galvanic cell and standard reduction potentials: Ag (aq) + e → Ag(s) E=0.80 V Pb²+ (aq) + 2e → Pb(s) E = -0.13 V IMA Which one of the following statements is TRUE? a) The cell on the left containing Ag (aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation...

  • Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e−...

    Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e− → Ag (s)   0.7996 Al3+ (aq) + 3e− → Al (s) −1.676 Au+ (aq) + e− → Au (s)   1.692 Au3+ (aq) + 3e− → Au (s)   1.498 Ba2+ (aq) + 2e− → Ba (s) −2.912 Br2 (l) + 2e− → 2Br− (aq)   1.066 Ca2+ (aq) + 2e− → Ca (s) −2.868 Cl2 (g) + 2e− → 2Cl− (aq)   1.35827 Co2+ (aq) + 2e−...

  • 6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e →...

    6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(aq)....

  • Use the standard half-cell potentials listed below to determine which the following metals will dissolve in...

    Use the standard half-cell potentials listed below to determine which the following metals will dissolve in hydrochloric acid. Cl2(g) + 2e + 2C1-(aq); E° = 1.36 V 2H+(aq) + 2e + H2(g); E° = 0.00 V O Cu; E°(Cu2+/Cu) = +0.34V O Au; E°(Au3+/Au) = +1.50V O Al; E°(A13+/Al) = -1.66V O Ag; E°(Ag+/Ag) = +0.80V O Pt; E°(Pt2+/Pt) = +1.19V

  • Use the standard half-cell potentials listed below to determine which the following metals will dissolve in...

    Use the standard half-cell potentials listed below to determine which the following metals will dissolve in hydrochloric acid. Cl2(g) + 2e -- 2014(aq); E° = 1.36 V 2H+(aq) + 2e - H2(g); E° = 0.00 V OPt; E°(P+2+/Pt) = +1.19V O Ag; E°(Ag+/Ag) = +0.80V O Au; EⓇ(Au3+/Au) = +1.50V O Al; E(A13+/Al) = -1.66V O Cu; E(Cu2+/Cu) = +0.34V

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT