Calculate the e.m.f of the following cell: Cd|Cd^(2+)(0.01M)||H^(+)(0.02M)|Pt,H_2(0.8atm) Given: E^@(Cd^(2+)|Cd)=-0.40V
Calculate the e.m.f. of the following cell at 298 K, Mg|Mg^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag
For the cell, Pt|Cl_2(g,0.4"bar")|Cl^(-)(aq,0.1M)"||"Cl^(-)(aq),0.01M)|Cl_2(g,0.2"bar")|pt
Determine the potential of the following cell: Pt|H_2(g,0.1 "bar")|H^+(aq,10^(-3)M"||"MnO_4^-)(aq),0.1M) Mn^(2+)(aq,0.01M),H^+(aq,0.01M)|Pt Given : E_(MnO_4^(-)|Mn^(2+))^(@)=1.51V
Calculate the emf of the following cell at 298k : Feabs(Fe^(2+)(0.001M)) abs(H^+(1M)) H_2(g)(1 b a r ),Pt(s) (given E^@,_(cell)=+0.44V )
Write The Nernst equation and calculate the e.m.f. of the following cell at 298K. Fe_((s))|Fe_((0.001M))^(2+)||H_((1M))^(+)|H_(2(1atm).Pt) Given E_(Fe^(2+)//Fe)^(@)=-0.44V
Calculate Delta_(r)G for the reaction at 27^(@)C H_(2)(g)+2Ag^(+)(aq)hArr2Ag(s)+2H^(+)(aq) Given : P_(H2)=0.5 bar, [Ag^(+)]=10^(-5)M, [H^(+)]=10^(-3)M,Delta_(r)G^(@)[Ag^(+)(aq)]=77.1kJ//mol
Calculate potential (EMF) of the cell Cd/ Cd2+ (0.01M) ||H+(0.02M) | H (0.5 atm) given E° for Cd2+/Cd = -0.40V