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 298 K ) Ag_((g)) // AgCl_((s)) // Cl_((aq))^(-) ||AgNO_(3(aq)) // Ag_((s)) Which of the following is correct ?

For the voltaic cell respresents below Ni(s) | Ni^(2+)(aq) || Ag^(+)(aq) | Ag(s) Which change will increase the cell potential?

for the electrochemical cell: Ag|AgCl(s)|KCl(aq)||AgNO_(3)(aq)|Ag . The overall cell reaction is

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]

Select the correct cell reaction of the cell Pt(s)|Cl_2(g)|Cl^(-)(aq)"||"Ag^+(aq)|Ag(s) :

Select the correct cell reaction of the cell Pt(s)|Cl_2(g)|Cl^(-)(aq)"||"Ag^+(aq)|Ag(s) :

Select the correct cell reaction of the cell Pt(s)|Cl_2(g)|Cl^(-)(aq)"||"Ag^+(aq)|Ag(s) :

The reaction, (1)/(2) H_(2) (g) + Ag Cl (s) = H^(+) (a.q) + Cl^(-) (a.q) + Ag (s) occurs in the galvanic cell: