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In a galvanic cell, the following reacti...

In a galvanic cell, the following reaction:
`Zn(s)+2Ag^(2+)(aq)toZn^(2+)(aq)+2Ag(s),E_(cell)^(@)=1.50V`
(a) Is the direction of flow of electrons from zinc to silver or silver to zinc?
(b) How will the concentration of `Zn^(2+)` ions and `Ag^(+)` ions be affected when the cell functions?

Text Solution

Verified by Experts

(a) Zn loses electrons while `Ag^(+)` ions in `Ag//Ag^(+)` electrons gais electrons. Hence, flow of electrons is from Z to Ag. ltBrgt (bgt Zn changes into `Zn^(2+)` ions. Hence, concentration of `Zn^(2+)` ions increases. `Ag^(+)` ions change into Ag. Hence, concentration of `Ag^(+)` ions keeps on decreasing.
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Knowledge Check

  • The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is

    A
    `2.6xx10^(49)`
    B
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    C
    `6.1xx10^(30)`
    D
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  • A galvanic cell involves the following reaction: Zn(s)+2Ag^(+) (aq.) hArr Zn^(2+) (aq.)+2Ag(s) Select the correct statements among the following :

    A
    Zinc is negatively charged
    B
    The given redox process is spontaneous
    C
    `Ag^(+) +e^(-) rarr Ag`, takes place at anode
    D
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  • If in a galvanic cell, the cell reaction is reversed as Cu(s)|Cu^(2+)(aq)||Zn^(+2)(aq)|Zn the cell potential will be

    A
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    D
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