The `E^(@)` at `25^(@)`C for the following reaction is 0.22 V. Calculate the equilibrium constant at `25^(@)`C :
`H_(2)(g)+2AgCl(s)to2Ag(s)+2HCl(aq)`

The E at 25^(@) C for the following reaction is 0.22 V. The equilibrium constant at 25^(@) C is very H_(2)(g) +2AgCl(s) rarr -2Ag (s)+2HCl(aq)

The E^@ at 25^@C for the following reaction is 0.22 V H_(2(g)) + 2AgCl_((s)) to 2Ag_((s)) + 2HCl_((aq)) . If the equilibrium constant at 25^@ C is 2.8 xx 10^(x) , x is

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s) E^(c-)._(cell)=0.46V

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s) E^(c-)._(cell)=0.46V

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s) E^(c-)._(cell)=0.46V

Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V

The emf of the following cell is 0.256 V at 25^@C and 0.2595 V at 35^@C. Calculate heat of reaction taking place at 25^@C. Pt(H_(2))|HCl(aq)||AgCl|Ag