At 298 K,the standard electrode potentials o | vedclass

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(C) The standard reduction potentials $(SRP)$ are given as: $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$,$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \ V$,$E^{\circ}_{Cu^{

Vedclass · Accepted Answer

$2CuSO_{4(aq)} + 2Ag_{(s)} \rightarrow 2Cu_{(s)} + Ag_2SO_{4(aq)}$

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(C) The standard reduction potentials $(SRP)$ are given as: $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$,$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \ V$,$E^{\circ}_{Cu^{2+}/Cu} = 0.34 \ V$,and $E^{\circ}_{Ag^{+}/Ag} = 0.80 \ V$. $A$ metal with a lower $SRP$ value can displace a metal with a higher $SRP$ value from its salt solution. Comparing the values,the reactivity order is $Zn > Fe > Cu > Ag$. In option $C$,$Ag$ is less reactive than $Cu$ $(E^{\circ}_{Ag^{+}/Ag} > E^{\circ}_{Cu^{2+}/Cu})$,therefore $Ag$ cannot displace $Cu$ from $CuSO_4$ solution. Thus,the reaction $2CuSO_{4(aq)} + 2Ag_{(s)} \rightarrow 2Cu_{(s)} + Ag_2SO_{4(aq)}$ is not spontaneous and cannot occur.

At $298 \ K$,the standard electrode potentials of $Cu^{2+}/Cu$,$Zn^{2+}/Zn$,$Fe^{2+}/Fe$ and $Ag^{+}/Ag$ are $0.34 \ V$,$-0.76 \ V$,$-0.44 \ V$ and $0.80 \ V$,respectively. On the basis of standard electrode potential,predict which of the following reactions cannot occur?

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