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

Calculate the equilibrium constant for the reaction 2Fe3+(aq) + 2I– (aq) → 2Fe2+(aq) + I2(s) E0cell = 0.236V

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)

Calculate the equilibrium constant for the reaction: Cd^(2+)+Zn(s)rarrZn^(2+)(aq)+Cd(s) If E_(Cd^(2+)|Cd)=-0.403V and E_(Zn^(2+)|Zn)=-.763V

Using the standerd half-cell potential listed, calculate the equilibrium constant for the reaction : Co(s)+2H^(+)(aq)toCo^(2+)(aq)+H_(2)(g)" at 298 K" Co^(2+)(aq)+2e^(-)toCo(s) E^(@)=-0.277 V

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 equilibrium constant for the reaction at 298K Cu(s)+Cl_(2)(g)toCuCl_(2)(aq) Given that R=8.314JK^(-1)mol^(-1) , E^(@)Cu^(2+)//Cu=0.34V , E^(@)(1)/(2)Cl_(2)//Cl^(-)=1.36V F=96500C" "mol^(-1)

Complete the reaction : Cu^(2+) (aq) + NH_3 (aq.) rarr

calculate the value of equilibrium constant (K_f) for the reaction: Zn^(2+)(aq)+4OH^(-)(aq)iffZn(OH)_4^(2-)(aq) Given: Zn^(2+)(aq)+2e^(-)toZn(s0,E^(@)=-0.76 V Zn(OH)_4^(2-)(aq)+2e^(-)toZn(s)+4OH^(-)(aq),E^(@)=-1.36 V 2.303(RT)/F=0.06

Calcualate the Delta_rG for the reaction: Mg(s)+Cu^(2+)(aq)rarrMg^(2+)(aq)+Cu(s) Given: E_(cell)^@=+2.71V, 1F=96500C mol^-1

Calculate the standard Gibbs energy for the given cell reaction :Zn(s)+Cu 2+ (aq)→Zn 2+ (aq)+Cu(s) E cell ​ =2.71V at 298K (Faraday's constant, F=96500 Cmol −1 )