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Calculate the e.m.f. of the cell in whic...

Calculate the e.m.f. of the cell in which the following reaction takes place: `Ni(s) + 2Ag^(+)(0.004 M) → Ni^(2+)(0.1 M) + 2Ag (s)` Given that `E^(@)`Cell =1.05V

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To calculate the e.m.f. of the cell for the given reaction, we will use the Nernst equation. The reaction is: \[ \text{Ni(s)} + 2\text{Ag}^+(0.004 \, \text{M}) \rightarrow \text{Ni}^{2+}(0.1 \, \text{M}) + 2\text{Ag(s)} \] ### Step 1: Identify the standard cell potential (E°cell) The standard cell potential is given as: \[ E^\circ_{\text{cell}} = 1.05 \, \text{V} \] ...
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Calculate the e.m.f. of the cell in which the following reaction takes place : Ni(s) +2Ag^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s) Given E_(cell)^(@) =1.05 v

Calculate the emf of the cell in which the following reaction takes place : Ni(s)+2Ag^(+)(0.002M) to Ni^(2+) (0.160M) +2Ag(s) Given that E_("cell")^(Theta)=1.05V

Knowledge Check

  • Calculate the emf of the following concentration cell at 25^(@)C : Ag(s)|AgNO_(3) (0.01 M)||AgNO_(3) (0.05 M)|Ag (s)

    A
    0.828V
    B
    0.0413V
    C
    `-0.0413` V
    D
    `-0.828` V

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