Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a)...

Question

Question

science chemistry

Answer 1

Similar Homework Help Questions

A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + N12+(aq) a) calculate the...

A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + N12+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode?
Part A Describe a galvanic cell that uses the reaction: 2Ag+ (aq) + Ni(s) + 2Ag(s)...

Part A Describe a galvanic cell that uses the reaction: 2Ag+ (aq) + Ni(s) + 2Ag(s) + Ni2+ (aq) Match the items in the left column to the appropriate blanks in the sentences on the right Reset Help Nja: Ag There is an anode in an aqueous solution of and an cathode in an aqueous solution of A connects the anode and cathode compartment. The electrodes are connected through an external circuit Ag semiconductor Ni salt bridge dielectric Write the...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The...

A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...

Calculate the standard cell potential (∆Eo) for the galvanic cell: Ni (s) 1 Ni2+ (aq) II...

Calculate the standard cell potential (∆Eo) for the galvanic cell: Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced...

Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced cathode half reaction b. write the balanced anode half reaction C. Write the balanced overall reaction d. Calculate E。, the cell potential. Is the reaction spontaneous as written? e Calculate Eolf [AP ] = 4.00 M, [Ni2+] = 2.00 x 10-5 M.
For the cell Ni(s) Ni2+(aq) || Ag+(aq) Ag(s), the standard cell potential is 1.03 V. A...

For the cell Ni(s) Ni2+(aq) || Ag+(aq) Ag(s), the standard cell potential is 1.03 V. A cell using these reagents was made, and the observed potential was 0.80 V at 25°C. What is a possible explanation for the observed voltage? The volume of the Agt solution was larger than the volume of the Ni2+ solution. The Agt concentration was larger than the Ni2+ concentration. The Ag electrode was twice as large as the Ni electrode. The Ni2+ concentration was larger...

6. Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) ? Ni2+(aq)...

6. Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) ? Ni2+(aq) + 2At– (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni) = –0.25 V]
For the reaction Ni2+(aq) + 2Fe2+(aq) ? Ni(s) + 2Fe3+(aq), the standard cell potential E°cell is

For the reaction Ni2+(aq) + 2Fe2+(aq) ? Ni(s) + 2Fe3+(aq), the standard cell potential E°cell is A. +2.81 V.B. +1.02 V.C. +0.52 V.D. -1.02 V.E. -2.81 V.Please show your steps, thank you :)
15) Consider a galvanic cell with a Ni electrode in 1.0 M Ni2+(aq) joined by a...

15) Consider a galvanic cell with a Ni electrode in 1.0 M Ni2+(aq) joined by a salt bridge to a silver electrode in 1.0 M Ag+(aq). Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is "dead". Answer: [Ag+] = 4.6 * 10-18 M, [Ni2+] = 1.5 M

In a galvanic cell, one half-cell consists of a nickel strip dipped into a 1.00 M...

In a galvanic cell, one half-cell consists of a nickel strip dipped into a 1.00 M solution of Ni(NO3)2. In the second half-cell, solid manganese is in contact with a 1.00 M solution of Mn(NO3)2. Ni is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 0.935 V at 25°C. (a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e-. Use the smallest integer...