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Calculate the EMF of cell Ni//Ni^(2+) ...

Calculate the EMF of cell
`Ni//Ni^(2+) (0.01M)"//"Cl^(-)0.1M//Cl_(2)`, Pt `E^(@)Ni^(2+)//Ni= -0.250V : E^(@)Cl_(2)//Cl^(-)= +1.360V`

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The correct Answer is:
`+1.73V`
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The e.m.f of the cell, Ni//Ni^(2+)(1M)////Cl^(-)(1M)//Cl_(2),Pt is E^(@)Ni^(2+)//Ni= -0.25V,E^(@)1//2Cl_(2)//Cl^(-)=1.36V

Calculate the EMF of the cell Cu//Cu^(2+)(0.1M)"//"Cl^(-) (0.01)// 1/2 Cl_(2) , Pt E^(@) Cu^(2+)//Cu = +0.33V E^(@) 1/2 Cl_(2)//Cl^(-) = +1.36V

Calculate electrode potential of Zn^(2+)(0.1M)//Zn"||"Cl^(-)(0.01)//Cl_(2), Pt E^(@)Zn^(2+)//Zn = -0.762V , E^(@) 1/2 Cl_(2)//Cl^(-) = + 1.36V

Calculate the EMF of Zn//Zn^(2+)(0.1)"//"Cu^(2+)(0.1)//Cu E^(@) of Zn^(2+)//Zn = 0.762V , E^(@) of Cu^(2+)//Cu = +0.337V

Calculate E of the cell with Cu^(2+) (0.1)//Cu electrode and Cl^(-)(0.1M)// 1/2Cl_(2) , Pt electrode. E^(@) Cu^(2+)//Cu= +0.33V and E^(@) 1/2 Cl_(2)//Cl^(-) = 1.36V

Calculate the EMF of the cell formd from Ag & Ni electrodes E^(@).Ag^(+)//Ag=(+0.799V) E^(@)Ni^(2+)//Ni= -0.250V

E^(@) values of Ni^(2+) , Ni and Cl_(2), Cl^(-) are respectively -0.25V and +1.37V . Calculate the EMF of the cell Ni, Ni^(2+) (0.01M)//Cl^(-)(0.1M), Cl_(2) , pt. Potential of nickel electrode is given as,

What is nernst equation. Calculate the EMF of the galvanic cell construted fro these electrodes. Zn//Zn^(2+) (1.0M)"||"Cu^(2+)(1.0M)//Cu E^(@)Zn^(2+)//Zn= -0.766V, E^(@)Cu^(2+)//Cu= +0.327V

For the cell , Hg,Hg_2 Cl_2//Cl (0.1M)//Cl^(-)(0.01M)//Cl_2, Pt E_("cell")^@ is 1.10V , Hence , E_("cell") is

Calculate the emf of the cell consisting the following half cells Al//Al^(3+)(0.001M), Ni//Ni^(2)(0.50M). Given that E_(Ni^(2+)//Ni)^(0)=-0.25V E_(Al^(3+)//Al)=-1.66V(log 8xx10^(-6)=-5.0969).

AAKASH SERIES-ELECTROCHEMISTRY -Subjective Exercise -3 (Short Answer Questions)
  1. How are the cells systemically represented ? Given examples.

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  2. E^@ values of Zn^(2+), Zn and Cu^(2+), Cu are respectively -0.76 V a...

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  3. The potential of the cell Cu, Cu^(2+) (0.1M)"//"HCl (xM), Cl(2), Ptis...

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  4. E^@ for Mg to 2e^(-) + Mg^(2+) is + 2.37 V and for Cu to 2e^(-) + Cu ...

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  5. E^(@) value of Co^(2+), Co, Al^(3+) , Al , Ag^(+), Ag and Ba^(2+), Ba ...

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  6. Two students use of the same stock solutions of zinc sulphate and a so...

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  7. Calculate the Electrode potential of single electrode. Cu^(2+)(0.01M)...

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  8. Standard reduction potential of I(3)^(-), I^(-) and Fe^(3+), Fe^(2+) ...

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  9. Calculate single electrode potential of Pt, Cl(2)//Cl^(-) (0.01)(E^(@...

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  10. Calculate the EMF of Zn//Zn^(2+)(0.1)"//"Cu^(2+)(0.1)//Cu E^(@) of Zn^...

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  11. Calculate the EMF of cell Ni//Ni^(2+) (0.01M)"//"Cl^(-)0.1M//Cl(2), ...

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  12. Calculate the EMF of the cell formd from Ag & Ni electrodes E^(@).Ag^...

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  13. Write the cell reactions of the cell fored from Sn^(2+)//Sn, Pb^(2+...

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  14. Calculate electrode potential of Zn^(2+)(0.1M)//Zn"||"Cl^(-)(0.01)/...

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  15. Calculate the EMF of the cell Cu//Cu^(2+)(0.1M)"//"Cl^(-) (0.01)// ...

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  16. What is nernst equation. Calculate the EMF of the galvanic cell constr...

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  17. Electrode potentials of Cu^(2+)//Cu and Ag^(+)//Ag electrodes are + ...

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  18. E^(@)Zn^(2+)//Zn = -0.77V. What is the 'E' value of the electrode cont...

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  19. Write the cell reactions for a) Ni//Ni^(2+)// //Cu^(2+)//Cu b) Cu...

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  20. Calculate E of the cell with Cu^(2+) (0.1)//Cu electrode and Cl^...

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