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 (at 298K) Ag(s) | AgCl(s) | Cl^(-)(aq)|| AgNO_(3)(aq) | Ag(s) Which of the following is correct?

For the cell (at 298K) Ag(s) | AgCl(s) | Cl^(-)(aq)|| AgNO_(3)(aq) | Ag(s) Which of the following is correct?

For the cell reaction, A(s) + 2B^(-)"(aq) rarr A^(2+) (aq) + 2B(s) , the value of Kc is 3.98 xx 10^(15) .Calculate E_(cell)^(@) at 298 K.

Calculate the simultaneous solubilities of AgSCN and AgBr . K_(sp) (AgSCN) = 1.0 xx 10^(-12), K_(sp) (AgBr) = 5.0 xx 10^(-13)

1/2 H_2(g)+AgCl(s)=H^+ (aq)+Cl^(-) (aq)+Ag(s) occurs in the galvanic cell:

The overall reaction electrochemical cell at 298K. Ag(s)|AgI(s)|I^(-)(aq)||Cl^(-)(aq)|Hg_(2)Cl_(2)|Hg(l)|Pt(s) [Given: E_(Cl^(-)|Hg_(2)Cl_(2)|Hg)^(@)=0.26V. E_(Ag^(+)|Ag)^(@)=0.8V . K_(sp)(Agl)=10^(-16) and (2.303RT)/(F)=0.06 ] E_("cell")^(@) of the above cell is:

The overall reaction electrochemical cell at 298K. Ag(s)|AgI(s)|I^(-)(aq)||Cl^(-)(aq)|Hg_(2)Cl_(2)|Hg(l)|Pt(s) [Given: E_(Cl^(-)|Hg_(2)Cl_(2)|Hg)^(@)=0.26V. E_(Ag^(+)|Ag)^(@)=0.8V . K_(sp)(Agl)=10^(-16) and (2.303RT)/(F)=0.06 ] At equilibrium ratio of ([Cl^(-)])/([I^(-)]) in the above cell will be:

The overall reaction electrochemical cell at 298K. Ag(s)|AgI(s)|I^(-)(aq)||Cl^(-)(aq)|Hg_(2)Cl_(2)|Hg(l)|Pt(s) [Given: E_(Cl^(-)|Hg_(2)Cl_(2)|Hg)^(@)=0.26V. E_(Ag^(+)|Ag)^(@)=0.8V . K_(sp)(Agl)=10^(-16) and (2.303RT)/(F)=0.06 ] The overall reaction occuring in the above cell is: