Home
Class 12
CHEMISTRY
For a cell reaction : M^(n+)(aq)+"ne"^(-...

For a cell reaction : `M^(n+)(aq)+"ne"^(-) to M(s)`, the Nernst equation for electrode potential at any concertation measured with respect to standard hydrogen electrode is represented as

A

`E_((M^(n+)//M))=E_((M^(n+)//M))^@-"RT"/"nF"ln (1/([M^(n+)]))`

B

`E_((M//M^(n+)))=E_((M//M^(n+)))^@-"RT"/"nF"ln (([M^(n+)])/([M]))`

C

`E_((M^(n+)//M))=E_((M^(n+)//M))^@-"RT"/"nF" "log" 1/([M])`

D

`E_((M^(n+)//M))=E_((M^(n+)//M^(n+)))^@-"RT"/"nF"ln [M^(n+)]`

Text Solution

Verified by Experts

The correct Answer is:
A
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS|Exercise Conductance Of Electrolytic Solutions|23 Videos

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS|Exercise Electrolytic Cells And Electrolysis|24 Videos

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS|Exercise Galvanic Cell|19 Videos

  • COORDINATION COMPOUNDS

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

  • GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

Similar Questions

Explore conceptually related problems

Write Nernst equation for the electrode reaction : M^(n+) + "ne"^(-) to M (s)

Write Nernst equation for the electrode reaction : M^(n+)(aq)+"n"e^(-)(aq) to M(s)

Knowledge Check

  • Assertion(A): The absolute value of the electrode potential cannot be determined experimentally Reason (R): The electrode potentials are generally determined with respect to standard hydrogen electrodes.

    A
    A and R are correct R is the correct explanation of A
    B
    A and R are correct R is not the correct explanation of A
    C
    A is correct, but R is worng
    D
    A is wrong, but R is correct

  • For the reaction: M^(n+)+ ne^(-) rarr M(s). The correct representation of Nernst equation is:

    A
    `E_(M^(n+)//M)=E _(M^(n+)//M)^(o) + (0.0591)/n log [Mn^(+)]`
    B
    `E_(M^(n+)//M)=E _(M^(n+)//M)^(o) -(0.0591)/n log [Mn^(+)]`
    C
    `E_(M^(n+)//M)=E _(M^(n+)//M)^(o) -n/(0.0591) log [Mn^(+)]`
    D
    None of these

  • For the reaction 2 A (s) + B^(2+) (aq) to 2 A^(+) (aq) + B(s) , Nernst equation for the EMF of the cell is

    A
    `E = E^(@) - (RT)/(2F) "ln" ([A^(+)])/([B^(2+)])`
    B
    `E = E^(@) - (RT)/(2F) "ln" ([A^(+)])/([B^(2+)]^(2))`
    C
    `E = E^(@) - (RT)/(F) "ln" ([A^(+)])/(sqrt([B^(2+)]))`
    D
    `E = E^(@) + (RT)/(F) "ln" ([A^(+)])/(sqrt([B^(2+)]))`

    • Similar Questions

    Explore conceptually related problems

    The Nernst equation for the potential of an electrode M_((aq))^(n+)|M_((s)) is _________.

    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 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: 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 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 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 reactions is not correct?

    Home
    Profile