Home
Class 12
CHEMISTRY
What will be the emf for the given cell ...

What will be the emf for the given cell ?
`Pt|H_(2)(g,P_(1))|H^(+)(aq)|H_(2)(g,P_(2))|Pt`

A

`(RT)/(F)log_(e)(p_(1))/(p_(2))`

B

`(RT)/(2F)log_(e)(p_(1))/(p_(2))`

C

`(RT)/(F)log_(e)(p_(2))/(p_(1))`

D

`(RT)/(2F)log_(e)^(p_(2))/(p_(1))`

Text Solution

Verified by Experts

The correct Answer is:
B
The `E^(@)` of cell will be zero.
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISRY

    RESONANCE ENGLISH|Exercise CBSE Problems|34 Videos

  • ELECTROCHEMISRY

    RESONANCE ENGLISH|Exercise Advanced Level Problems|88 Videos

  • ELECTROCHEMISRY

    RESONANCE ENGLISH|Exercise Exercise 3|7 Videos

  • ELECTRO CHEMISTRY

    RESONANCE ENGLISH|Exercise PHYSICAL CHEMITRY (ELECTROCHEMISTRY)|53 Videos

  • EQUIVALENT CONCEPT & TITRATIONS

    RESONANCE ENGLISH|Exercise Part -IV|22 Videos

Similar Questions

Explore conceptually related problems

Which of the following changes will increase the EMF of the cell : Co(s)|CoCl_(2)(M_(1))||HCl(M_(2))||(H_(2),g)Pt

Which of the following changes will increase the EMF of the cell : Co(s)|CoCl_(2)(M_(2))||HCl(M_(2))||(H_(2),g)Pt

Write the cell reaction for each of the following cells. Pt,H_(2)(g)|H^(+)(aq)|Ag^(+)(aq)|Ag(s)

At 25^(@)C, DeltaH_(f)(H_(2)O,l) =- 56700 J//mol and energy of ionization of H_(2)O(l) = 19050J//mol . What will be the reversible EMF at 25^(@)C of the cell, Pt|H_(2)(g) (1atm) |H^(+) || OH^(-) |O_(2)(g) (1atm)|Pt , if at 26^(@)C the emf increase by 0.001158V .

Consider the cell : Pt|H_(2)(p_(1)atm)|H^(o+)(x_(1)M) || H^(o+)(x_(2)M)|H_(2)(p_(2)atm)Pt . The cell reaction be spontaneous if

Which of the following changes will increase the emf of the cell : Co(s)| CoCl_(2) (M_1) || HCl(M_2) | pt(H_(2), g)

The correct Nernst equation for the given cell Pt_((s)) | Br_(2(l)) | Br^(-) (M) || H^(+) (M) |H_(2(g)) (1bar) | Pt_((s)) is

calculate the e.m.f (in V) of the cell: Pt|H_2(g)|BOH(Aq)"||"HA(Aq)|H_2(g)|Pt , 0.1bar 1M 0.1M 1bar Given : K_a(HA)=10^(-7), K_b(BOH)=10^(-6) (a)0.39V (b)0.36V (c)0.93V (d)None of these

What is the unit of K_(p) for the reaction ? CS_(2)(g)+4H_(2)(g)hArrCH_(4)(g)+2H_(2)S(g)

Galvanic cells generate electrical energy at the expense of a spontaneous redox reaction. In an electrode concentration cell two like electrodes having different concentrations, either because they are gas electrodes operating at different pressures or because they are amalgams (solutions in mercury) with different concentrations are dipped into the same solution. Eg. An example is a cell composed of two chlorine electrodes with different pressure of Cl_(2) : Pt_(L)|Cl_(2)(P_(L))|HCl(aq)|Cl_(2)(P_(R))|Pt_(R) Where P_(L) and P_(R) are the Cl_(2) pressure at the left and right electrodes. Calculate the EMF of the electrode concentration cell represented by : Hg-Zn(c_(1))|Zn^(+2)(aq)|Hg-Zn(c_(2)) At 25^(@)C.c_(1)=2g of Zn per 100g of Hg and c_(2)=1g of Zn per 50g of Hg

Knowledge Check

  • The correct Nernst equation for the given cell Pt_((s)) | Br_(2(l)) | Br^(-) (M) || H^(+) (M) |H_(2(g)) (1bar) | Pt_((s)) is

    A
    `E_"cell"=E_"cell"^@-"0.0591"/2 "log" ([Br_(2(l))][H_2])/([H^+]^2[Br^-]^2)`
    B
    `E_"cell"=E_"cell"^@-"0.0591"/2 "log" ([H^+]^2[Br^-]^2)/([Br_(2(l))][H_2])`
    C
    `E_"cell"=E_"cell"^@-"0.0591"/2 "log" ([H^+]^2[H_2])/([Br_(2(l))][Br^(-)]^2)`
    D
    `E_"cell"=E_"cell"^@-"0.0591"/2 "log" ([Br_(2(l))][Br^-]^2)/([H^+]^2[H_2])`
    • RESONANCE ENGLISH-ELECTROCHEMISRY-Part 2
    1. What will be the emf for the given cell ? Pt|H(2)(g,P(1))|H^(+)(aq)|...

      Text Solution

      |

    2. Which reaction is possible at anode?

      Text Solution

      |

    3. For a cell given below: Ag|Ag^(+)||Cu^(2+)|Cu Ag^(+)+e^(-)toAg,E^(...

      Text Solution

      |

    4. Conductance (Siemens, S) is directly proportional to the area of the v...

      Text Solution

      |

    5. At 25^(@)C, the standard emf of a cell having reaction involving two e...

      Text Solution

      |

    6. Standard reduction electrode potentials of three metals A,B and C are ...

      Text Solution

      |

    7. Consider the following E^@ values . E(Fe^(3+)//Fe^(2+)^@ = + 0.77 V, ...

      Text Solution

      |

    8. The limiting molar conductivities overset(o)(wedge) for NaCl, KBr an...

      Text Solution

      |

    9. In a cell that utilises the reaction ZN(s)+ 2H^(+)(aq)rightarrow Zn^(2...

      Text Solution

      |

    10. The E(M^(3+)//M^(2+))^(@) values for Cr, Mb, Fe and Co are -0.41, +1.5...

      Text Solution

      |

    11. The highest electrical conductivity of the following aqueous solution ...

      Text Solution

      |

    12. Aluminium oxide may be electrolysed at 1000^(@)C to furnish aluminium ...

      Text Solution

      |

    13. The molar conductivities, ^^(NaOAc)^(oo) and ^^(HCI)^(@) at infinite d...

      Text Solution

      |

    14. Given the data at 25^(@)C, Ag((s)) +I((aq))^(-) rarr AgI((s)) +e^(-)...

      Text Solution

      |

    15. Resistance of a conductivity cell filled with a solution of an electro...

      Text Solution

      |

    16. The equivalent conductances of two strong electrolytes at infinite dil...

      Text Solution

      |

    17. The cell : (Zn|Zn^(2+)(1M)|| Cu^(2+)(1M)|Cu) (E(cell)^(@)= 1.10V),wa...

      Text Solution

      |

    18. Given: E(Cr^(3+)//Cr)^(@) =- 0.72 V, E(Fe^(2+)//Fe)^(@) =- 0.42V. The ...

      Text Solution

      |

    19. Given : E(Fe^(3+)//Fe)^(@) = -0.036V, E(FE^(2+)//Fe)^(@)= -0.439V. The...

      Text Solution

      |

    20. The Gibbs energy for the decomposition of Al2O3 at 500^@C is as follow...

      Text Solution

      |