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Define standard electrode potential....

Define standard electrode potential.

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Standard electrode potential is the electrode potential of an electrode when all the species involved in the given half-cell (or electrode reaction) are in their standard states with reference to standard hydrogen electrode.
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The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Which of the following oxides will be themally most stable?

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Which of the following metals will not displace hydrogen from water?

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Given the standard reduction potentials. E_(K^(+)//K)^(@)=-2.93V, E_(Ag^(+)//Ag)^(@)=+0.80V, E_(Hg^(+)//Hg)^(@)=0.79V E_(Mg^(+)//Mg)^(@)=-2.37V, E_(Cr^(3+)//Cr)^(@)=-0.74V The correct increasing order of reducing power is:

Which cell will measure standard electrode potential of copper electrode?

The positive value of the standard electrode potential of Cu^(2+)//Cu indicates that.......

Calculate the standard potential of the cell ,If the standard electrode potentials of Zn^(2+)//Zn and Ag^(+) //Ag are -0.763 V and + 0.799 V respectively .

If the standard electrode poten tial of Cu^(2+)//Cu electrode is 0.34V. What is the electrode potential of 0.01 M concentration of Cu^(2+) ?

The potential associated with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0.0 volt. The electrode potential value for each electrode process is a measure of relative tendency of the active species in the process to remain in the oxidised/reduced form. A negative E^(@) means that the redox couple is a stronger reducing agent than the H^(+)//H_(2) couple. A positive E^(@) means that the redox couple is a weaker reducing agent than the H^(+)//H_(2) couple. The metal with greater positive value of standard reduction potential forms the oxide of greater thermal stability. Which of the following reactions is not correct ?

The potential associated with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0.0 volt. The electrode potential value for each electrode process is a measure of relative tendency of the active species in the process to remain in the oxidised/reduced form. A negative E^(@) means that the redox couple is a stronger reducing agent than the H^(+)//H_(2) couple. A positive E^(@) means that the redox couple is a weaker reducing agent than the H^(+)//H_(2) couple. The metal with greater positive value of standard reduction potential forms the oxide of greater thermal stability. Which of the following couples will have highest value of emf ?

Consult the table of standard electrode potential and suggest three substances that can oxidize Fe^(2+) ions under suitable conditions.

ICSE-ELECTROCHEMISTRY-EXERCISE (PART-II Descriptive Questions)
  1. Give two functions of salt bridge.

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  2. Define electrode potential, oxidation potential and reduction potenti...

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  3. Define standard electrode potential.

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  4. Define standard electrode potential.

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  5. What is standard hydrogen electrode ? Give the reaction that occurs a...

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  6. Standard electrode potential of SHE at 298 K is :

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  7. What is the emf of the cell when the cell reaction attains equilibriu...

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  8. What does the standard electrode potential of a metal being negative (...

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  9. In the operation of a galvanic cell, at one of the electrodes, oxidat...

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  10. What is the representation of a Daniell cell ?

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  11. What does the negative value of E("cell")^(Theta) indicate?

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  12. The standard reduction potential for Zn^(2+)//Zn is -0.76V. Write th...

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  13. Write Nernst equation for the following cell reaction : Zn"|"Zn^(2+)...

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  14. What is the effect of increase in concentration of zinc ions on the e...

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  15. How can the reduction potential of an electrode increased ?

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  16. Under what conditions will a galvanic cell send no current into outer...

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  17. Electrochemical Series

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  18. Write the symbolic notation for standard hydrogen electrode and its p...

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  19. Write Nernst equation for the electrode reaction: M^(n+) +n e^(-) t...

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  20. Write Nernst equation for the reaction: (i) 2Cr(s) +3Cd^(2+)(aq) to...

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