The equilibrium constent of the reaction. Cu(s)+2Ag(aq). Leftrightarrow Cu^(2+) (aq.)+2Ag(s) E^(@)=0.46" V at 298 K is"
Calculate equilibrium constant for the reaction at 25^(@)C Cu(s)+2Ag^(+)(aq) hArr Cu^(2+)(aq)+2Ag(s) E^(@) value of the cell is 0.46 " V " .
The equilbrium constant for the reaction : Cu + 2 Ag^(+) (aq) rarr Cu(2+) (aq) +2 Ag, E^@ = 0. 46 V at 299 K is
Calculating the thermodynamic equilibrium constant from the cell emf : The standard emf for the following galvanic cell is 0.46 V Cu(s)|Cu^(2+)(aq.)||Ag^(+)(aq.)|Ag(s) Calculate the equilibrium cosntant K_(C) for the reaction Cu(s)+2Ag^(+)(aq.)hArr Cu^(2+)(aq.)+2Ag(s) Strategy : Substitute the standard emf into the Equation (3.9) realting this quantity to the thermodynatmic equilibrium constant, K_(eq.). Solve K_(eq.). Note that K_(eq.). = K_(C^(.))
Given the equilibrium constant : K_(c) of the reaction : Cu(s) + 2Ag^(+)(aq) rightarrow Cu^(2+) (Aq) + 2Ag(s) is 10xx10^(15) , calculate the E_(cell)^(@) of this reaction at 298K . ([2.303 (RT)/(Ft) at 298K = 0.059V])
The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is
Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V
