[" 36.The equilibrium constant for the following reaction at "25^(@)C" is "2.9times10^(9)" .Calculate standard "],[" voltage of the cell."]

The equilibrium constant for the following reaction at 25^(@)C " is " 2.9 xx 10^(9) . Calculate standard voltage of the cell. C1_(2(g)) + 2Br_((aq))^(-) hArr Br_(2(1)) + 2C1_((aq))^(-)

The equilibrium constant for the following reaction at 25^(@)C is 2.9×10^(9) . Calculate standard voltage of the cell . Cl_2(g)+Br_(aq)^(-) ⇌ Br_2(l)+2Cl_(aq)^(-)

The equilibrium constant for the following reaction at 25^@C is 2.9 xx 10^9 . Calculate standard voltage of the cell. Cl_(2(g)) +Br_(aq)^- narr Br(2(i))+2CI_((aq))^- .

Calculate the equilibrium constant for the following reaction at 25^@C . Ag^(+)(aq) + Fe^(2+)(aq) to Ag(s) + Fe^(3+)(aq) The standard emf of the corresponding voltaic cell is 0.03 V.

The value of equilibrium constant K_p for the reaction CO(g)+H_2O(g) leftrightarrow CO_2(g)+H_2(g) is 1.06 times 10^5 at 25^@C Calculate standard free energy change of the reaction at the same temperature.