Short AnswerMake your own galvanic cell. Choosea pair of electrodes (anode & cathode)from the table of standard reductionpotential and compute the cell potentialand delta G of your galvanic cell. Is thisspontaneous? Why? Short AnswerUsing the same galvanic cell you havechosen, compute the cell potential anddelta G of your galvanic cell when theconcentration of your solution in Anode is2.0 M while your cathode is 1.5 M and thetemperature is 25 degrees Celsius. Is thisspontaneous? Why?

In galvanic cell chemical energy is converted to electrical energy. Here we have to choose two…

Make your own galvanic cell. Choose a pair of electrodes (anode & cathode) from the table of standard reduction potential and compute the cell potential and delta G of your galvanic cell. Is this spontaneous? Why?

Make your own galvanic cell. Choose a pair of electrodes (anode & cathode) from the table of standard reduction potential and compute the cell potential and delta G of your galvanic cell. Is this spontaneous? Why?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The cell made from an anode half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a cathode half-cell consisting of a nickel electrode in 0.25 M nickel(II) nitrate solution. Determine the cell potential (Ecell)
A galvanic (voltaic) cell consists of an inert platinum clectrode in a solution containing 1.0 M tin(IV) ion and 1.0M tin(II) ion, and another inert platinum clectrode in a solution containing 1.0 M iron(III) ion and 1.0M iron(II) ion, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found in the standard reduction potentials table. E: cell V
Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)
The following spontaneous reaction occurs when metallic zinc is dipped into a solution of copper sulfate. Zn (s) +Cu^ 2+ (aq) ----> Zn^ 2+ (aq) +Cu (s) Describe a galvanic cell that could take advantage of this reaction. What are the half-cell reactions? Make a sketch of the cell and label the cathode and anode, the charges on each electrode , the direction of ion flow, and the direction of electron flow .
A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Excell V
A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00 x 10–4 M in the two half-cells. The reduction potential of Ni2+ is –0.23 V. Calculate the potential of the cell at 25°C.
Explain the following relationships: Delta G and w, cell potential and w, cell potential and Delta G, cell potential and Q. Using these relationships, explain how you could make a cell in which both electrodes are the same metal and both solutions contain the same compound, but at different concentrations. How could this cell run spontaneously?
A galvanic (voltaic) cell consists of an electrode composed of manganese in a 1.01.0 M manganese(II) ion solution and a second electrode composed of lead in a 1.01.0 M lead(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 ∘C25⁢ ∘C. Use this list of standard reduction potentials.
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. V 'cell II
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of copper in a 1.0 M copper(I) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E cell || = V
A galvanic (voltaic) cell contains a copper cathode immersed in a copper(I) chloride solution and a nickel anode immersed in a nickel(II) chloride solution. The two solutions are connected with a salt bridge. Write the balanced equation for the galvanic cell. Phases are optional. balanced equation: A current of 2.40 A is observed flowing through the cell for a period of 2.81 h. Calculate the amount of charge flowing through the circuit during this time. C Calculate the number of moles of electrons flowing through the circuit during this time. moles of clectrons: Calculate the mass change in grams of the copper and nickel electrodes. mass change of copper clectrodc: mass change of nickel electrode:
. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?