Given: `E_(Sn^(2+)//Sn) ^0 = -0.14V` , `E_(Pb^(2+)//Pb) ^0 = -0.13V`. Determine `[(Sn^(2+))//(Pb^(2+))]` at equilibrium. For cell reaction `Sn |Sn^(2+) || Pb^(2+) | Pb` , Take `(2.303RT)//F = 0.06V`

Write the cell reaction for the cell Sn"|"Sn^(2+)"||"Au^(3+)"|"Au

Correct order of SN2 reaction is :

For an electrochemical cell Sn(s)Sn^(2+) (aq,1M)||pb^(2+) (Aq,1M)|Pb(s) the ratio ([Sn^(2+)])/([Pb^(2+)] when this cell attians equilibrium is_______ (Given : E_(sn^(2+)|Sn)^(@) = -0.14V, E_(pb^(2+|Pb^(@))= -0.13V, (2.303RT)/(F = 0.06))

If E_(Sn^(2+)//Sn)^(@)=-0.14V, what would be the value of E_(Sn//Sn^(2+))^(@) ?

Given : E^(@) (Cu^(2+//Cu) = 0.337V and E^(@) (Sn^(2+//Sn) = -0.136V . Which of the following statements is correct?

Calculate the equilibrium constant K_(c) for the rections. 3Sn^(4) + 2 cr to 3Sn^(2+) + 2Cr^(3+) Given E^(o) = 0.885 V .

Consider the following E^@ values . E_(Fe^(3+)//Fe^(2+)^@ = + 0.77 V , E_(Sn^(2+)//Sn)^@=- 0.14 V The E_(cell)^@ for the reaction , Sn (s) + 2Fe^(3+)(aq) rarr 2 Fe^(2+)(aq)+ Sn^(2+)(aq) is ? (a) -0.58 V (b) -0.30 V (c) +0.30V (d) +0.58 V

For a cell involving one electron E_(cell)^(0)=0.59V and 298K, the equilibrium constant for the cell reaction is: [Given that (2.303RT)/(F)=0.059V at T=298K ]

Which of the following are SN^2 reactions ?

Answer, whether under standard conditions, the following reactions are possible or not: (i) Will copper reduce Ag^(+) " to " Ag ? Given E_(Ag^(+)//Ag)^(@) = 0.799 " volt" , E_(Cu^(2+)//Cu)^(@) = - 0.337 volt (ii) Will Fe^(3+) be reduced to Fe^(2+) by Sn^(2+) ions? given {:(Fe^(3+) | Fe^(2+) = 0.771 " volt"),(Sn^(2+) |Sn^(4+) = - 0.250 " volt"):} (iii) would you use a silver spon to stir a solution of Cu(NO_(3))_(2) ?