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

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^(Θ) ? R=8.314 J K^(-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?

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) ):

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.

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))

The standard e.m.f of a cell, involving one electron change is found to be 0.591 V at 25^(@) C . The equilibrium constant of the reaction is : (F=96,500C mol^(-1) : R=8.314 Jk^(-1)mol^(-1)

Calculate DeltaG^@ for the reaction 2HCl (g) + F_2(g) to 2HF (g) + Cl_2(g) at 25^@C at Given : Delta_f G^@ [ HCl (g)] = -95.30 kJ mol^(-1) . Delta_fG^@ [ HF(g)] = -273 kJ mol^(-1) . Also calculate the equilibrium constant the reacton at 25^@C . Given, gas constant R = 8.314 JK^(-1) mol^(-1) .

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .