AgBr (s) `harr` `Ag^(+)`(aq) + `Br^(-)`(aq); `E^(@)`= `-0.72V` If the value of `K_(sp)` at `25^(@)C` is `10^(-b)` then the value of "b" is Use `(2.303RT)/(F)`= 0.06 )

EMF of the following cell is 0.6 volt. Ag (s) | AgBr ( s) | KBr (0.01 m) |AgNO_(3) ( 0.001M) | Ag( s) K_(sp) of AgBr is expressed as 1 xx 10^(-x) , x is [Take ( 2.303RT)/(F ) = 0.06 V ]

For the galvanic cell: Ag(s) | AgBr(aq) | Br^(-)(aq) || Cl^(-)(aq)| AgCl(s)| Ag(s) the value of E_(cell)^(@) at 298 K: [Given : K_(sp) of AgCl =2 xx 10^(-10) . K_(sp) of AgBr = 4 xx 10^(-13) = (2.303R xx 298)/(F) = 0.06 , log 2 = 0.3]

For the cell Cu (s) | Cu ^(2+) (aq) (0.1 M) || Ag ^(+) (aq) (0.01 M) | Ag (s) the cell potential E _(1) = 0.3095 V For the cell Cu (s) | Cu ^(+2) (aq) (0.01 M) || Ag ^(+) (aq)( 0. 001 M) | Ag (s) the cell potential = _______ xx 10 ^(-2) V. (Round off the Nearest Integer). [Use : (2.303 RT)/(F) =0.059 ]

Given : BaF_(2) (s) harr Ba^(+2) (aq)+2 F^(-) (aq); K_(sp) = 1.0times10^(-8) M^(3) HF(aq) harr H^(+) (aq)+ F^(-) (aq); K_(a) = 6.5times10^(-6) M The value of K_(c) for BaF_(2) (s)+ 2H^(+)(aq) harr Ba^(+2)(aq) + 2HF(aq) is:

10Cl^(-)(aq) + 2MnO_(4)^(-)(aq) + 16H^(+)(aq) rightarrow 5Cl_(2)(g) + 2Mn^(2+0()aq) + 8H_92)O(l) The value of E^(@) for this reaction at 25^(@)C is 0.15 V. What is the value of K for this reaction?

Given the equilibrium constant : K_(c) of the reaction : Cu(s) + 2Ag^(+)(aq) rightarrow Cu^(2+) (Aq) + 2Ag(s) is 10xx10^(15) , calculate the E_(cell)^(@) of this reaction at 298K . ([2.303 (RT)/(Ft) at 298K = 0.059V])