The `DEltaG^@` for the Daniell cell has been found to be -212.3 kJ at `25^@C`. Calculate the equilibrium constant for the cell reaction.

The standard emf of a galvanic cell involving cell reaction with n = 2 is formed to be . 0.295 V at 25^(@)C . The equilibrium constant of the reaction would be :

Calculate the standard cell potentials of galvanic cell in which the following reactions take place: Calculate the Delta_rG^ o and equilibrium constant of the reactions. 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq)+ 3Cd

Calculate the standard cell potentials of galvanic cell in which the following reactions take place: Calculate the Delta_rG^o and equilibrium constant of the reactions. Fe^(2+)(aq) + Ag^+ (aq) rarr Fe^(3+) (aq) + Ag(s)

The resistance of a conductivity cell with 0.1 M KCl solution is found to be 200 ohm at 298K. When the same cell was filled with 0.02 M NaCl solution, the resistance at the same temperature is found to be 1100 ohm . Calculate: the cell constant of the cell in m^-1 . Given conductivity of 0.lM KCl is 1.29 Sm^(-1) ]

The resistance of 0.5N solution of an electrolyte ina conductivity cell was found to be 25Omega . Calculate the equivalent conductivity of the solution if the electrodes in the cell are 1.6cm apart & having an area of cross section 3.2cm^(2)

The cell in which the following reaction occurs: 2Fe^(3+)(aq)+2I^(-)(aq)rarr2Fe^(2+)(aq)+I_2(s) has E_(cell)^o=0.236 V at 298 K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

The equilibrium constant (K_(c)) for the reaction 2HCl(g)hArrH_(2)(g)+CL_(2)(g) is 4xx10^(-34) at 25^(@)C .what is the equilibrium constant for the reaction ? (1)/(2)H_(2)(g)+(1)/(2)Cl_(2)(g)hArrHCl(g)

Two reactions of the same order have equal pre-exponential factors but their activation energies difter by 24.9 kJ mol^-1 . Calculate the ratio between the rate constants of these reactions at 27^@C . (Gas constant, R= 8.3 JK^-1 mol^-1 ).