Calculate the equilibrium constant for the cell reaction :
`4Br^(-)+O_(2)+4H^(+)rarr2Br_(2)+2H_(2)O."Given "E_(cell)^(@)=0.16 V`

Calculate the value of the equilibrium constant of the given reaction at 298 K: 4Br^(-)+O_(2)+4H^(+)rarr 2Br_(2)+2H_(2)O Given : E_("cell")^(@)=+0.16V

For the cell reaction 4Br^(-) + O_(2)+4H^(+) rarr Br_(2)+2H_(2)O E_("cell")^(@)=0.16 V , the value of log K_(c) is :

Calculate the equilibrium constant for the reaction at 298K 4 Br + O2 + 4H+ → 2 Br2 + 2H2O Given that Ecell = 0.16V​

Calculate the equilibrium constant for the reaction: 3Sn(s) +2Cr_(2)O_(7)^(2-) +28 H^(+) rarr 3Sn^(+4) +4Cr^(3+) +14H_(2)O E^(@) for Sn//Sn^(+2) = 0.136 V E^(@) for4 Sn^(2+)//Sn^(4+) =- 0.154V E^(@) for Cr_(2)O_(7)^(2-)//Cr^(3+) = 1.33V

Calculate the equilibrium constant for the reaction: 3Sn(s) +2Cr_(2)O_(7)^(2-) +28 H^(+) rarr 3Sn^(+4) +4Cr^(3+) +14H_(2)O E^(@) for Sn//Sn^(+2) = 0.136 V E^(@) for4 Sn^(2+)//Sn^(4+) =- 0.154V E^(@) for Cr_(2)O_(7)^(2-)//Cr^(3+) = 1.33V

Calculate the equilibrium constant for the reaction: 3Sn(s) +2Cr_(2)O_(7)^(2-) +28 H^(+) rarr 3Sn^(+4) +4Cr^(3+) +14H_(2)O E^(@) for Sn//Sn^(+2) = 0.136 V E^(@) for4 Sn^(2+)//Sn^(4+) =- 0.154V E^(@) for Cr_(2)O_(7)^(2-)//Cr^(3+) = 1.33V

Calculate the equilibrium constant for the following cell reaction. (1)/(2)Cl_(2) (g) +Br^(-) to (1)/(2) Br_(2) (l) +Cl^(-) , E^(Theta) =0.30V