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[" What is the emf at "25^(@)C" for the cell,Ag,"|[" AgBr "(s),Br^(-)],[a=0,34]|[Fe^(3+),Fe^(2+)],[a=0,1],a=0,02|Pt],[" The standard reduction potentials for the half-reactions "AgBr+e^(-)rarr Ag+Br^(-)" and "Fe^(3+)+e^(-)rarr Fe],[" are "+0.0713V" and "+0.770" V respectively."],[[" (A) "0.474" volt "," (B) "0.529" volt "," (C) "0.356" volt "," (D) "0.713volt]]

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what is the emf at 25^(@)C for the cell, Ag|{:(AgBr(s)" " Br^(-)), (" "alpha = 0.34):}||{:(Fe^(3+) " " Fe^(2+)), (alpha = 0.1 " " alpha = 0.02):}|Pt The standard reduction potentials for the half-reactions AgBr + e^(-) rightarrow Ag + Br^(-) and Fe^(3+) + e^(-) rightarrow Fe^(2+) are +0.0713V and +0.770V respectively.

what is the emf at 25^(@)C for the cell, Ag|{:(AgBr(s)" " Br^(-)), (" "alpha = 0.34):}||{:(Fe^(3+) " " Fe^(2+)), (alpha = 0.1 " " alpha = 0.02):}|Pt The standard reduction potentials for the half-reactions AgBr + e^(-) rightarrow Ag + Br^(-) and Fe^(3+) + e^(-) rightarrow Fe^(2+) are +0.0713V and +0.770V respectively.

The standard reduction potentials E^@ for the half reactions are as Zn=Zn^(2+)+2e, E^@=+0.76V Fe=Fe^(2+)+2e, E^@=+0.41V the emf of the cell reaction, Fe^(2+)+Zn=Zn^(2+)+Fe is

Calculate the standard e.m.f. of the reaction Fe^(3+)+3e^(-)rarrFe_((s)) . Given the e.m.f. values of Fe^(3+)+e rarr Fe^(2+) and Fe^(2+)+2e rarr Fe_((s))" as "+0.771 V and =0.44V " respectively."

Calculate the standard e.m.f. of the reaction Fe^(3+)+3e^(-)rarrFe_((s)) . Given the e.m.f. values of Fe^(3+)+e rarr Fe^(2+) and Fe^(2+)+2e rarr Fe_((s))" as "+0.771 V and =0.44V " respectively."

The standard electrode potantials of the half cells Ag^(+)//Ag and Fe^(3+),Fe^(2+)//Pt are 0.7991V and 0.771V respectively. Calculate the equilibrium constant of the reaction : Ag_((s))+Fe^(3+)hArr Ag^(+)+Fe^(2+)