The equilibrium constant for a reaction is 10 .What will be the value of `Delta G^(Theta)?` R=`8.314JK^(-1)` `mol^(-1)`,T=300K .

The equilibrium constant for a reaction is 10 . What will be the value of DeltaG^(Θ) ? R=8.314 J K^(-1) mol^(-1), T=300 K .

The equilibrium constant for a reaction is 100 what will be the value of DeltaG^(@) ? R=8.314JK^(-1)mol^(-1),T=300 K :-

The equilibrium constant for a reaction is 10. What will be the value of DeltaG^@ ? R = 8.314 J K^(-1) mol^(-1), T = 300K.

The equilibrium constant for a reaction is 100 what will be the value of ΔG^∘ at 300K?

Certain reaction is at equilibrium at 82^(@)C and Delta H for this reaction is 21.3 kJ mol^(-1) . What would be the value of Delta S(in JK^(-1) mol^(-1)) for the reaction.

A reaction is at equilibrium at 100^(@)C and the enthalpy change for the reaction is "42.6 kJ mol"^(-1) . What will be the value of DeltaS in "J K"^(-1)"mol"^(-1) ?

The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25^(@)C . The equilibrium constant of the reaction would be (Given F=96,500 C mol^(-1), R = 8.314 JK^(-1) mol^(-1) ):

For a reaction, K_p = 1.8 xx 10^(-7) at 300K. What is the value of DeltaG^@ at this temeprature ? (R =8.314 J K^(-1) mol^(-1))

If the standard electrode potential for a cell is 2V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu^(2+) (aq) at 300 k is approximately : (R=8JK^(-1) mol^(-1) , F= 96000 mol^(-1))

Calculate equilibrium constant for the reaction given below at 400K , if DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) PCI_(5)(g) rarr PCI_(3)(g) +CI_(2)(g)