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What is nernst equation. Calculate the E...

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`

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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 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

The emf of galvanic cell of the reaction Zn+Cu^(2+)rarr Zn^(2+) + Cu is (E^(@)Zn^(2+)//Zn " is" -0.76V " and " Cu^(2+)//Cu " is " +0.34V)

Calculate the Electrode potential of single electrode. Cu^(2+)(0.01M)//Cu" "(E^(@)= +0.337V)

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 K_(c) for the reaction at 298 K Zn_((s))+Cu_((aq))^(+2)hArrZn _((aq))^(2+)+Cu_((s)) E _(Zn^(2+)//Zn)^(0)=-0.76V, E_(Cu^(2+)//Cu)^(0) =+0.34V.

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

E^@ values of Zn^(2+), Zn and Cu^(2+), Cu are respectively -0.76 V and + 0.34 . Calculate the EMF of the cell Zn//Zn^(2+) (0.1M)"//"Cu^(2+)(0.1 M)//Cu .

Define emf. Calculat the emf of the following galvanic cell : Zn_((s))+Cu_((aq))^(+2)to Zn_((aq))^(+2)+Cu_((s)) E_(zn^(+2//Zn))^(0) =0.76V(anode) ,E_(cu^(+3//Cu))^(0)=+0.34 (Cathode)

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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