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To find the standard potential of M^(3+)...

To find the standard potential of `M^(3+)//M` electrode , the following cell is constituted : `Pt|M|M^(3+((.001moLL^(-1)|| Ag ^(+) ((0.01moLL^(-1))|` Ag. The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction `M^(3+)+ 3e^(-) to M` at 298 K will be :
(Given `E_(Ag^(+)//Ag^(@)` at 298 K = 0.80 Volt)

A

(0.32Volt)

B

(0.66Volt)

C

(0.38VOlt)

D

(1.28Volt)

Text Solution

AI Generated Solution

To find the standard potential of the half-reaction \( M^{3+} + 3e^- \rightarrow M \) at 298 K, we can follow these steps: ### Step 1: Write the Nernst Equation The Nernst equation relates the cell potential (E) to the standard electrode potential (\( E^0 \)) and the concentrations of the reactants and products: \[ E_{cell} = E^0_{cell} - \frac{0.059}{n} \log Q \] where \( n \) is the number of moles of electrons transferred, and \( Q \) is the reaction quotient. ...
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To find the standard potential of M^(3+)//M electrode, the following cell is constituted: Pt|M |M^(3+) (0.0018 mol^(-1)L)||Ag^(+) (0.01mol^(-1)L)|Ag The emf of this cell is found to be 0.42 volt. Caldulate the standard potential of the half reaction M^(3+) +3e^(-) to M. E_(Ag^(+)//Ag)^(@)=0.80volt

To find the standard potential of M^(3+)//M electrode, the following cell is constituted : Pt|M|M^(3+) (0.0018 mol^(-1) L)||Ag^(+) (0.01 mol^(-1) L(|Ag The emf of this cell is found to be 0.42 volt. Calculate the standard potential of the half reaction M^(3+)+3e^(-) rarr M . E_(Ag^(+)//Ag)^(@)=0.80 volt.

Knowledge Check

  • The standard electrode potential of the electrode Ag(s) , AgCl| KCl (1 M) is

    A
    `+0.2225 V`
    B
    `+0.2245 V`
    C
    `+0.2255 V`
    D
    `0.2265 V`

  • The electrode potential of a silver electrode dipped in 0.1 M AgNO_(3) solution at 298K is (E^(@) red of Ag =0.80 volt)

    A
    0.0741 V
    B
    0.0591 V
    C
    0.741 V
    D
    0.859 V

  • The EMF of the following cell is 0.86 volts Ag|AgNO_(3)(0.0093M)||AgNO_(3)(xM)|Ag . The value of x will be

    A
    82.8M
    B
    2.28M
    C
    0.228M
    D
    1.14M

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    Converting measured potentials to standard potentials: In investigating the properties of rare and expensive metal such as rhenium (Z = 75) , it is both impractical and uneconomical to prepare cells with standard concentrations. The find the standard potential of the Re^(3+)(aq.)//Re(s) electrode, the following cell is constructed: Pt(s) | Re(s)| Re^(3+)(aq., 0.018 M)|| Ag^(+)(aq., 0.010 M) | Ag(s) The potential of this cell is found to be 0.42 V with the Re electrode as the node. Calculate the standard potential of the half reaction Re^(3+)(aq.)+3e^(-)hArrRe(s) Strategy: Table 3.1 lists the E_(@) for the Ag^(+)(aq.) | Ag(s) electrode as 0.80 . We can find the E^(@) of the other electrode by finding the E^(@) of the cell through the application of the Nernst equation.

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