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A voltaic cell is constructed from an Ni2+ (aq) -Ni(s) half-cell and an Ag+ (aq)- Ag(s)...
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...
A voltaic cell is made from Ni(s), Ni2+(aq), Ag(s) and Ag+ a. Fill in the diagram...
A voltaic cell is made from Ni(s), Ni2+(aq), Ag(s) and Ag+
a. Fill in the diagram with the chemicals associated with each
part of the cell.
b. Write a balanced cell reaction
A voltaic cell is made from Ni(s), Niz*(aq), Ag(s) and Ag 7. a. Fill in the diagram with the chemicals associated with each part of the cell. Ni2+ + 2 e-→ Ni(s) Ag+ + e-→ Ag(s) -0.25 0.80
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.60molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V Part A What is the initial cell potential? Part B What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? Part C What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s)....
A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s). What is the emf of this cell when [Ni2+]=2.80 M and [Zn2+]= 0.120 M ? What is the emf of the cell when [Ni2+]=0.280 M and [Zn2+]= 0.960 M ?
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.80 molL−1 and 0.130 molL−1, respectively. Zn2+(aq)+2e−→Zn(s)E∘=−0.76V Ni2+(aq)+2e−→Ni(s)E∘=−0.23V A) What is the cell potential when the concentration of Ni2+ has fallen to 0.600 molL−1? B) What are the concentrations of Ni2+ and Zn2+ when the cell potential falls to 0.45 V?
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]
If you construct a Galvanic / Voltaic cell using a Ni(s) / Ni2+(aq) half cell and...
If you construct a Galvanic / Voltaic cell using a Ni(s) / Ni2+(aq) half cell and an Al(s)/ Al3+(aq)half cell,and connect the whole cell to a voltmeter by connecting the Al half cell to the positive terminal of the voltmeter, what will be the display?
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni...
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ 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: + + The cathode reaction is: + V> + The net cell reaction is:...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 °C. The...
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 °C. The initial concentrations of Ni2+ and Zn2+ are 1.00 M and 0.150 M respectively. a. What is the initial cell potential? b. What is the cell potential when the concentration of Ni2+ has fallen to 0.250 M? (Hint: What should the concentration of Zn2+ be if Ni2+ has fallen from its original concentration to its current concentration?)
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3...
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.9 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag (aq). E® Zn/Zn2+ = -0.763 V Eº Ag/Ag+ = 0.7994 V Concentration = Submit Answer Try Another Version 6 item attempts remaining
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...
A voltaic cell is made from Ni(s), Ni2+(aq), Ag(s) and Ag+
a. Fill in the diagram with the chemicals associated with each
part of the cell.
b. Write a balanced cell reaction
A voltaic cell is made from Ni(s), Niz*(aq), Ag(s) and Ag 7. a. Fill in the diagram with the chemicals associated with each part of the cell. Ni2+ + 2 e-→ Ni(s) Ag+ + e-→ Ag(s) -0.25 0.80
Enter electrons as e A voltaic cell is constructed in which the anode is a Ni Ni2+ half cell and the cathode is a Hg|Hg2+ 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: + + The cathode reaction is: + V> + The net cell reaction is:...
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.9 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag (aq). E® Zn/Zn2+ = -0.763 V Eº Ag/Ag+ = 0.7994 V Concentration = Submit Answer Try Another Version 6 item attempts remaining
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