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Identify, with a reason, the stronger ox...

Identify, with a reason, the stronger oxidising agent in each of the following pairs.
`Cr^(3+),Fe^(2+)`
`["Given : "E_((1)/(2)Cl_(2)(g)|Cl^(-))^(@)=+1.36V, `
`E_((1)/(2)Br_(2)(l)|Br^(-))^(@)=+1.07V,`
`E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.80V,`
`E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Fe^(2+)|Fe)^(@)=-0.44V,`
`E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Cr^(3+)|Cr)^(@)=-0.74V]`

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`Fe^(3+)` is stronger oxidant than `Cr^(3+)`
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Find the stronger oxidising agent in each pair, stating reason. (d) Cr^(3+), Fe^(3+) "Given : "E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V, E_((1)/(2)Br_(2)|Br^(-))^(@)=+1.07V, E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.80V, E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Fe^(2+)|Fe)^(@)=-0.44V , E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Cr^(3+)|Cr)^(@)=-0.74V

Find the stronger oxidising agent in each pair, stating reason. (c) Ag^(+), Cu^(2+) "Given : "E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V, E_((1)/(2)Br_(2)|Br^(-))^(@)=+1.07V, E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.80V, E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Fe^(2+)|Fe)^(@)=-0.44V , E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Cr^(3+)|Cr)^(@)=-0.74V

Find the stronger oxidising agent in each pair, stating reason. (a) Cl_(2), Br_(2) "Given : "E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V, E_((1)/(2)Br_(2)|Br^(-))^(@)=+1.07V, E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Ag^(+)|Ag)^(@)=+0.80V, E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Fe^(2+)|Fe)^(@)=-0.44V , E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Cr^(3+)|Cr)^(@)=-0.74V

Are the following reactions spontaneous? (a) Fe+Mg^(2+)rarr Fe^(2+)+Mg "Given : "E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Mg^(2+)|Mg)^(@)=-2.37V, E_(Cd^(2+)|Cd)^(@)=-0.40V, E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V

Using the data find out the strongest reducing agent - E_(Cr_(2)O_(7)^(2-)|Cr^(+))^(@)=+1.33V, E_(Cl_(2)|Cl^(-))^(@)=+1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=+1.51V, E_(Cr^(2+)|Cr)^(@)=-0.74V

Are the following reactions spontaneous? (b) Cd+Cl_(2)rarr Cd^(2+)+2Cl^(-) "Given : "E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Mg^(2+)|Mg)^(@)=-2.37V, E_(Cd^(2+)|Cd)^(@)=-0.40V, E_((1)/(2)Cl_(2)|Cl^(-))^(@)=+1.36V

Calculate the value of the equilibrium constant of the following reaction at 298 K: Given: E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Cl_(2)|2Cl^(-))^(@)=+1.36V

Fe has a much lower tendency to get oxidised than Mn and Cr - explain. [Given : E_(Cr^(2+)|Cr)^(0)=-0.9V, E_(Cr^(3+)|Cr^(2+))^(0)=-0.4V E_(Mn^(2+)|Mn)^(0)=-1.2V, E_(Mn^(3+)|Mn^(2+))^(0)=+1.5V E_(Fe^(2+)|Fe)^(0)=-0.4V, E_(Fe^(3+)|Fe^(2+))^(0)=+0.8V ]

Stability of Fe^(3+) ion is greater than Mn^(3+) ion but less than Cr^(3+) - explain. [Given : E_(Cr^(2+)|Cr)^(0)=-0.9V, E_(Cr^(3+)|Cr^(2+))^(0)=-0.4V E_(Mn^(2+)|Mn)^(0)=-1.2V, E_(Mn^(3+)|Mn^(2+))^(0)=+1.5V E_(Fe^(2+)|Fe)^(0)=-0.4V, E_(Fe^(3+)|Fe^(2+))^(0)=+0.8V ]

Given that, E_(Zn^(2+)|Zn)^(@)=-0.76V, E_(Cu^(2+)|Cu)^(@)=+0.34V , E_(Ni^(2+)|Ni)^(@)=-0.25V and E_(Ag^(+)|Ag)^(@)=+0.80V Which metal ions are reduced by Ag^(+) ?

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