[Pt|H_(2)(1atm)|HCl(0.01M)||AgCl(s)|A_(!)],[" at "298K
" if "/_G_(1)^(@)" values are at "25^(@)C],[
-109.56(kJ)/(mol)" for "AgCl(s)" and "
],[-130.79(kJ)/(mol)" for "(H^(+)+Cl^(-))(ag)

Calculate the cell EMF in mV for Pt|H_(2)(1atm)|HCl(0.01M)||AgCl(s)|Ag(s) at 298 K if triangleG_(1)^(@) values are at 25^(@)C -109.56(kJ)/(mol) for AgCl(s) and -130.79(kJ)/(mol) for (H^(+)+Cl^(-))(ag) (A). 456 mV (B). 654 mV (C). 546 mV (D). None of these

Calcualte the cell EMP in mV for Pt|H_(2)(1 atm) | HCl(0.01 M)|| AgCl(s)| Ag(s) at 298 K If DeltaG_(f)^(@) values are at 25^(@)C , -109.56 (kJ)/(mol) for AgCl(s) and -130.79 (kJ)/(mol) for (H^(+) + Cl^(-)(aq) , Take 1F = 96500 C

In the cell Pt(s)|H_(2)(g,1bar)|HCl (aq)| AgCl(s)|Ag(S)|Pt(s) the cell potential is 0.92V when a 10^(-6) mola1 HCl Ssolution is used. The standard electrode potential of (ACl//Ag,Cl^(-)) electrode is : {given, (2.30Rt)/(F) = 0.6V at 298K}

In the cell Pt(s)|H_(2)(g,1bar)|HCl (aq)| AgCl(s)|Ag(S)|Pt(s) the cell potential is 0.92V when a 10^(-6) mola1 HCl Ssolution is used. The standard electrode potential of (ACl//Ag,Cl^(-)) electrode is : {given, (2.30Rt)/(F) = 0.6V at 298K}

For the following cell reaction, Ag | Ag^(+) | AgCl | Cl^(-) | Cl_(2) , Pt Delta G_(f)^(0) (AgCl) =-109 kJ//mol Delta G_(f)^(0) (Cl ) = -129kJ//mol Delta G_(f)^(0) (Ag^(+)) = 78 kJ//mol E^@ of the cell is

Calculate DeltaG^(0) for the reaction H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l) at 298K. Given, at 298K DeltaH_(f)^(0) for H_(2)O(l) is -286 kJ *mol^(-1) and the molar entropies (S^(0)) for H_(2)(g),O_(2)(g) and H_(2)O(l) are 130.7, 205.1 and 69.9 J*K^(-1)*mol^(-1) respectively.

Calculate the equilibrium constant for the following reaction at 298K and 1 atmospheric pressure: C(grap hite) +H_(2)O(l) rarr CO(g) +H_(2)(g) Given Delta_(f)H^(Theta) at 298 K for H_(2)O(l) =- 286.0 kJ mol^(-1) for CO(g) =- 110.5 kJ mol^(-1) DeltaS^(Theta) at 298K for the reaction = 252.6 J K^(-1) mol^(-1)

Calculate the equilibrium constant for the following reaction at 298K and 1 atmospheric pressure: C(graphite) +H_(2)O(l) rarr CO(g) +H_(2)(g) Given Delta_(f)H^(Theta) at 298 K for H_(2)O(l) =- 286.0 kJ mol^(-1) for CO(g) =- 110.5 kJ mol^(-1) DeltaS^(Theta) at 298K for the reaction = 252.6 J K^(-1) mol^(-1)