Question

Given: Ag+(aq) + e-→Ag(s)    E° = +0.799 V Cr3+(aq) + e-Cr2+(aq.) Eo= - 0.41 V Ni2+(aq)...

Given:

Ag+(aq) + e-→Ag(s)    E° = +0.799 V

Cr3+(aq) + e-Cr2+(aq.) Eo= - 0.41 V

Ni2+(aq) + 2 e-→Ni(s) E° = -0.267 V

Generate two voltaic cells using the above 3 reactions. Show the anode and cathode half-reactions and the overall cell reactions and calculate Eo cell values.

Homework Answers

Answer #1

At cathode high reduction value equation will occur

Ag+ + e = Ag (s). E° = 0.799 V

At anode low reduction value will occur

Cr3+(aq) = Cr2+(aq) + e. E° = 0.41 V

Net cell reaction

Ag+(aq) + Cr3+(aq) = Ag(s) + Cr2+(aq) E° = 0.799 + 0.41 = 1.209 V

2. Ni2+(aq) + 2e = Ni(s) E° = -0.267 V

2Cr2+(aq) = 2 Cr3+(aq) + 2e E°= 0.41 V

Net cell reaction

Ni2+(aq) + 2 Cr2+(aq) = 2Ni(s) + 2 Cr3+(aq)

E° = 0.41 + ( -0.267 )

= 0.143 V

If you have any questions please comment

If you satisfied with the solution please rate it thanks

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A voltaic cell is constructed in which the anode is a Cr2+|Cr3+ half cell and the...
A voltaic cell is constructed in which the anode is a Cr2+|Cr3+ half cell and the cathode is a Ag|Ag+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: __(aq)(s)(l)(g) + __(aq)(s)(l)(g) -----> __(aq)(s)(l)(g) + __(aq)(s)(l)(g) The cathode reaction is: __(aq)(s)(l)(g) + __ (aq)(s)(l)(g) ----->   __(aq)(s)(l)(g) + __(aq)(s)(l)(g)...
A voltaic cell is constructed from an Ni2+(aq)−Ni(s) half-cell and an Ag+(aq)−Ag(s) half-cell. The initial concentration...
A voltaic cell is constructed from an Ni2+(aq)−Ni(s) half-cell and an Ag+(aq)−Ag(s) half-cell. The initial concentration of Ni2+(aq) in the Ni2+−Ni half-cell is [Ni2+]= 1.00×10−2 M . The initial cell voltage is +1.12 V . a. By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell. b. Will the concentration of Ni2+(aq) increase or decrease as the cell operates? c. What is the initial concentration of Ag+(aq) in the Ag+−Ag half-cell?
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The...
Assume you are constructing a Galvanic cell based on the half-reactions between Zn2+(aq)/Zn(s) and Ag+(aq)/Ag. The standard reduction potentials are given below. Ag+ (aq) + e- Ag (s) Eo = 0.80 V Zn2+ (aq) + 2 e- Zn(s) Eo = -0.76 V Write a balanced chemical REDOX equation and determine the Eo for the cell. What will be observed at the cathode and at the anode? Is the reaction thermodynamically favored? Explain.
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) +...
Au3+(aq) + 3e- --> Au(s) 1.498 V Ag+(aq) + e- --> Ag(s) 0.767 V Cu2+(aq) + 2e- --> Cu(s) 0.342 V Ni2+(aq) + 2e- -->Ni(s) -0.257 V Calculate the potential at 25ºC for the following cell: Cu | Cu2+ [0.024M] || Ag+ [0.0048M] | Ag
Write the cell notation for an electrochemical cell consisting of an anode where Ni(s) is oxidized...
Write the cell notation for an electrochemical cell consisting of an anode where Ni(s) is oxidized to Ni2+(aq) and a cathode where Fe3+(aq) is reduced to Fe2+(aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar. Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq) and a cathode where Ag+(aq) is reduced to Ag (s) . Assume...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo =...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo = 0.34 V MnO4 - (aq) + 4 H+ (aq) + 3 e- -----> MnO2 (s) + 2 H2O (l) Eo = 1.68 V A. What is the standard cell potential for a voltaic cell comprised of these two half reactions? B. What is the equilibrium constant for this reaction at 25 oC? C. How is the magnitude of the equilibrium constant consistent with a...
Consider the following half-reactions: Ag+ (aq) + e- --> Ag(s) E cell = 0.80 VV Cu2+(aq)...
Consider the following half-reactions: Ag+ (aq) + e- --> Ag(s) E cell = 0.80 VV Cu2+(aq) + 2e- --> Cu(s) E cell = 0.34 V Pb2+(aq) + 2e- --> Pb(s) E cell = -0.13 V Fe2+(aq) + 2e- --> Fe(s) E cell = -0.44 V Al3+ (aq) + 3e- --> Al(s) E cell = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)? a. Ag+(aq) and Cu2_(aq) b. Ag(s) and Cu(s) c. Fe2+(aq) and Al3+(aq) d....
Pb+2 +2e- ---> Pb(s) Eo= -0.13V Ag+ + le- ---> Ag(s) Eo= +.80V Pb(s)| Pb2+ (1M)...
Pb+2 +2e- ---> Pb(s) Eo= -0.13V Ag+ + le- ---> Ag(s) Eo= +.80V Pb(s)| Pb2+ (1M) || Ag+ (1M) | Ag(s) Determine which of the following statements about the cell shown are True or False. Cations move to the silver half-cell. The standard cell potential, ξo, equals 1.73 V. As the reaction proceeds, the concentration of the lead ions decreases. The cell, as represented by the line notation, is a galvanic cell. The lead half-cell is the anode. The mass...
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V...
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Ni -0.257 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are...
A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that...
A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). Write out the half-reactions occurring and state which reaction is occurring at the anode and which is occurring at the cathode. Please explain mathemcatically and in words. Thanks!
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT