Consider the following electrochemical cell: Zn(s) | Zn2+ (? M) ‖ Ni2+ (0.059 M) | Ni(s)...

Question

Question

Consider the following electrochemical cell: Zn(s) | Zn2+ (? M) ‖ Ni2+ (0.059 M) | Ni(s) Ecell = 0.51 V Determine the unknown quantity.

How to solve this question?

Answer 1

Similar Homework Help Questions

Consider the following electrochemical cell: Zn(s) | Zn2+ (? M) ‖ Ni2+ (0.025 M) | Ni(s)...

Consider the following electrochemical cell: Zn(s) | Zn2+ (? M) ‖ Ni2+ (0.025 M) | Ni(s) Ecell = 0.49 V Determine the unknown quantity. How to solve this question???
Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq)...

Consider the voltaic cell and reduction half potentials: Zn(s) | Zn 2+(aq) (0.100 M) || Ni2+(aq) (1.50 M) | Ni(s) Zn 2+ (aq)/Zn (s) E o = - 0.760 V Ni2+ (aq)/Ni (s) E o = - 0.230 V a) Sketch the voltaic cell represented with the above line notation. Label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution. Also indicate the direction of electron flow (3 marks). b)...
A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The...

A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.700 M and 0.120 M , respectively. The volume of half-cells is the same. Question 2 1 pts A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25°C. The initial concentrations of Ni2+ and Zn2+ are 1.700 M and 0.120 M, respectively. The volume of half-cells is the same. What is the concentration...

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?
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+ anode and a Ni/Ni2+ cathode at 25 ∘C. The...

A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.700 M and 0.120 M , respectively. The volume of half-cells is the same. What is the concentration of Ni2+ when the cell potential falls to 0.457 V ? Enter your answer to 4 decimal places and in units of mM.
A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The...

A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are 1.80 M and 0.120 M , respectively. The volume of half-cells is the same. Part A What is the concentrations of Ni2+ when the cell potential falls to 0.46 V ? Express your answer using one significant figure. Part B What is the cell potential when this voltaic cell is "dead"? Part C What is the concentration...
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?)

Calculate the voltage generated by the following cell. Zn(s)|Zn2+ (0.1M) || Ni2+(0.005M) |+ Ni(s) A. Write...

Calculate the voltage generated by the following cell. Zn(s)|Zn2+ (0.1M) || Ni2+(0.005M) |+ Ni(s) A. Write the overall cell redox equation. B. Label the anode and the cathode in the cell notation above. C. Calculate the standard cell potential. D. Use the Nernst equation to calculate the cell potential.