(a) When a bright silver object is placed in the solution of gold chloride, it acquires a golden tings but nothing happens when it is placed in solution of copper chloride. Explain this behaviour of silver.
[Given : `E_(Cu^(2+//)Cu)^(@)=+0.34 V, E_(Ag^(+//)Ag)^(@) =+0.80 V, E_(Au^(3+//)Au)^(@) =+1.40V`]
(b)
Consider the figure given above and answer the following questions :
(i) What is the direction of flow of electrons?
(ii) Which is anode and which is cathode?
(iii) What will happen if the salt bridge is removed ?
(iv) How will concentration of `Zn^(2+)` and `Ag^(+)` ions be affected when the cell functions ?
(v) How will concentration of these ions be affected when the cell becomes dead ?

Explanation

(a) When a bright silver object is placed in gold chloride

`E_("Cell")^(@) = E_("cathode")^(@) - E_("anode")^(@)`
`E_("cell")^(@) = E_(Au3+//Au)^(@)-E_(Ag+//Ag)^(@)`
= 1.40 - 0.80 = 0.60V
`E_("cell")^(@) = + 0.60V`
When silver is palced in copper chloride solution

`E_("cell")^(@) = E_(C)^(@) - E_(A)^(@)`
`=E_(Cu2+//Cu)^(@)-E_(Ag+//Ag)^(@) = 0.34 - 0.80`
`E_("cell")^(@) = - 0.46V`
As `E^(@)` cell is positive for gold chloride solution. Hence reaction is feasible and silver object acquires a golden tings but `E^(@)` cell is negative for copper chlrodie. Hence, nothing happens with it.
(b) (i) Electrons flow from negative pole to positive pole (from left to right) i.e., from anode to cathode.
(ii) The Zinc electrode at which oxidation takes place is anode and silver electrode wherer reduction takes places is cathode.
(iii) Circuit will not be completed, flow of electrons will stop and hence the current stops flowing.
(iv) Concentration of `Zn^(2+)` decreases and `Ag^(+)` ions increases when the cell functions.
(v) When E cell = 0, equilibrium is reached and concentration of `Zn^(2+)` and `Ag^(+)` ions will not change.