Interpretation:
Direction of flow of electrons in a Daniel cell is the reverse of the direction of the movement of anions. The reason for the contradictory situation has to be explained.
Concept Introduction:
Galvanic cell is an
Redox reactions are the reactions in which both oxidation and reduction takes place simultaneously. Oxidation is the removal electron from an atom or ion. Oxidation process increases the oxidation number. Reduction is the addition of electron to an atom or ion. Reduction process decreases the oxidation number. The electrochemical reaction in a Daniel cell is an example of
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- Electrochemical Cells II Consider this cell running under standard conditions: Ni(s)Ni2(aq)Cu+(aq)Cu(s) a Is this cell a voltaic or an electrolytic cell? How do you know? b Does current flow in this cell spontaneously? c What is the maximum cell potential for this cell? d Say the cell is connected to a voltmeter. Describe what you might see for an initial voltage and what voltage changes, if any, you would observe as time went by. e What is the free energy of this cell when it is first constructed? f Does the free energy of the cell change over time as the cell runs? If so, how does it change?arrow_forwardGive the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?arrow_forwardDetermine the overall reaction and its standard cell potential at 25 C for these reactions. Is the reaction spontaneous at standard conditions? Assume the standard reduction for Br2(l) is the same as for Br2(aq).. Pt(s)|H2(g)|H+(aq)Br2(aq),Br(aq)|Pt(s)arrow_forward
- As an example of an electrolytic cell, the text states: Sodium chloride is electrolyzed commercially in an apparatus called the Downs cell to produce sodium and chlorine. This is a high-temperature operation; the electrolyte is molten NaCl. Write the half-reaction equations for the changes taking place at each electrode. Is the electrode at which sodium is produced the anode or the cathode? The Downs cell electrolyzes molten melted sodium chloride, producing sodium and chlorine.arrow_forwardDetermine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?arrow_forwardDetermine the overall reaction and its standard cell potential at 25 C for this reaction. Is the reaction spontaneous at standard conditions? Cu(s)|Cu2+(aq)Au3+(aq)|Au(s)arrow_forward
- The following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25Varrow_forwardA potassium chloride solution is electrolyzed by passing a current through the solution using inert electrodes. A gas evolves at each electrode, and there is a large increase in pH of the solution. Write the half-reactions that occur at the anode and at the cathode.arrow_forwardHalf-cells were made from a nickel rod dipping in a nickel sulfate solution and a silver rod dipping in a silver nitrate solution. The half-reactions in a voltaic cell using these half-cells were Ag+(aq)+eAg(s)Ni(s)Ni2+(aq)+2e Sketch the cell and label the anode and cathode, showing the corresponding electrode reactions. Give the direction of electron flow and the movement of cations.arrow_forward
- For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mg(s)+Ni2+(aq)Mg2+(aq)+Ni(s) (b) 2Ag+(aq)+Cu(s)Cu2+(aq)+2Ag(s) (c) Mn(s)+Sn(NO3)2(aq)Mn(NO3)2(aq)+Sn(s) (d) 3Fe(NO3)2(aq)+Au(NO3)3(aq)3Fe(NO3)3(aq)+Au(s)arrow_forwardIs it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 Varrow_forward
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