Calculate the e.m.f. of the following cell at 298K:
`2Cr(s)+3Fe^(2+)(0.1M)to2Cr^(3+)(0.01M)+3Fe(s)`
Given: `E_((Cr^(3+)//Cr))^(@)=-0.74V,E_((Fe^(2+)//Fe))^(@)=-0.44V`.

Calculate e.m.f. of the following cell at 298 K, 2Cr(s)+3Fe^(2+)(0.1 M) to 2Cr^(3+)(0.01 M)+3Fe(s) ("Given" : E_((Cr^(3+)//Cr))^(@)=-0.74" V ", E_((Fe^(2+)//Fe))^(@)=-0.44" V ")

What is the value of E^(@) cell in the following reaction? Cr|Cr^(3+) (0.1 M)||Fe^(2+) (0.01 M)|Fe Given, E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V

Calculate the e.m.f. of the cell, Cr//Cr^(3+)(0.1 M) || Fe^(2+)(0.01 M)//Fe "Given" : E_(Cr^(3+)//Cr)^(@)=-0.75" V ", E_(Fe^(2+)//Fe)^(@)=-0.45" V " "Cell reaction" : 2Cr(s)+3Fe^(2+)(aq) to 2Cr^(3+)(aq)+3Fe(s) {"Hint". E_(cell)=E_(cell)^(@)-(0.0591V)/(6)"log"([Cr^(3+)]^(2))/([Fe^(2+)]^(3)}

Calculate the emf of the following cell at 298K : Fe(s)|Fe^(2+)(0.001M)||H^+(1M)|H_2(g)(1"bar"),Pt(s) (Given E_("Cell")^@=+0.44V)

Calculate E_(cell)^(@) for the following reaction at 298 K : 2 Cr (s ) + 3 Fe^(2+) (0.01 M) to 2 Cr^(3+) (0.01 M) + 3 Fe (s) Given : E_(cell) = 0.261 V

Calculate the potential of the following half - cells | cells : a. Cr|Cr^(3+)(0.1 M)||Fe^(2+)(0.01M)|Fe Given : E^(c-)._(Cr^(3+)|Cr)=-0.74V E^(c-)._(Fe^(2+)|Fe)=-0.44V b. 6e^(c-)+BrO_(3)^(c-)(aq)+3H_(2)OrarrBr^(c-)(aq)+6OH(aq) Given :E^(c-)._((BrO_(3)^(c-)|Br^(c-)))=0.61V, [BrO_(3)^(c-)]=2.5xx10^(-3)M,[Br^(c-)]=5.0xx10^(-3)M,pH=9.0 c. Ag|Ag^(o+)(0.1M)||Cl^(c-)(0.02M)|Cl_(2)(g)(0.5atm)|Pt Given E_((Ag^(o+)|Ag))=0.80V,E^(c-)((Cl_(2)|2Cl^(c-))=1.36V d. NO_(3) ^(c-)(aq)+2H^(o+)(aq)+e^(-)rarrNO_(2)+H_(2)O Given : E^(c-)._(NO_(3)^(c-)|NO_(2)=0.78V What will be the reductino potential of the half cell in neutral solution ? Assuming all the other species to be at unit concentration.