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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^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s)`
Given `E_(cell)^(@)`=1.05 v

Text Solution

AI Generated Solution

To calculate the e.m.f. (electromotive force) of the cell for the given reaction: \[ \text{Ni(s) + 2Ag}^+ \text{(0.002 M)} \rightarrow \text{Ni}^{2+} \text{(0.160 M) + 2Ag(s)} \] we will use the Nernst equation. The standard cell potential (\( E^\circ_{\text{cell}} \)) is given as 1.05 V. ### Step-by-Step Solution: 1. **Identify the half-cell reactions:** - **Anode (oxidation):** ...
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Explore conceptually related problems

Calculate the emf 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 that: E_("cell")^(@) = 1.05 V

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

Knowledge Check

  • Calculate emf of the cell in which the following reaction takes place :- Ni_(s) + 2Ag^(+) (0.002M) to Ni^(+2) (0.160M) + 2Ag_((s)) Given : E_("cell")^(o) = 1.05V, (2.303RT)/(F) = 0.06, log2 = 0.3

    A
    `1.05 V`
    B
    `0.912 V`
    C
    `1.19 V`
    D
    `2.05 V`

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