Delta G^(0) and Delta H^(0) for a reaction at 300K is -66.9kJmol^(-1) and -41.8kJmol^(-1) respectively Delta S^(0) for the same reaction at 300K is

triangleG^@ and triangleH^(@) for a reaction at 300K are -66.9 kJ/mole and 41.8 kJ/mole respectively. triangleG^(@) for the same reaction at 330K is

If Delta G^(@)gt 0 for a reaction then :

If the equilibrium concentration of the components in a reaction A+B hArr C+D are 3,5,10 and 15 mol L^(-1) respectively then what is Delta G^(@) for the reactiona at 300K ?

Delta H and Delta S for the reaction, Ag_(2)O(s)to 2A(s)+(1)/(2)O_(2)(g) , are 30.56 kJ mol^(-1) and 66.0 J mol^(-1) respectively. Calculate the temperature at which this reaction will be at equilibrium. Predict whether the forward reaction will be favoured above or below this temperature.

The standard Gibbs energies (Delta_(f)G^(Theta)) for the formation of SO_(2)(g) and SO_(3)(g) are -300.0 and -371.0 kJ mol^(-1) at 300K , respectively. Calculate DeltaG and equilibrium constant for the following reaction at 300K :

The values of DeltaH and DeltaS for two reactions are given below: Reaction A : DeltaH =- 10.0 xx 10^(3)J mol^(-1) DeltaS = +30 J K^(-1) mol^(-1) Reaction B: DeltaH =- 11.0 xx 10^(3)J mol^(-1) DeltaS =- 100J K^(-1) mol^(-1) Decide whether these reactions are spontaneous or not at 300K .

Consider an electrochemical cell : A(s)|A^(n+) (aq. 2M)||B^(2n+) (aq. 1M)|B(s) . The value of DeltaH^(@) for the cell reaction is twice that of DeltaG^(@) at 300 K. If the amf of the cell is zero, the DeltaS^(@) ("in "JK^(-1) mol^(-1)) of the cell reaction per mole of B formed at 300 K is ______ . (Given : In (2) = 0.7, R (universal gas constant) = 8.3 J K^(-1) mol^(-1) . H, S and G are enthalpy, entropy and Gibbs energy, respectively.)

If Delta H gt 0 and Delta S gt 0 , the reaction proceeds spontaneously when :-

For the reaction at 300 K , A(g) rarr B(g) + E(g), DeltaH^(@) = -30 KJ mol^(-1) , the decrease in standard entropy is 0.1 KJK^(-1)mol^(-1) .The equilibrium constant K for the reaction is ________.

The standard electrode potential E^(@) and its temperature coefficient ((dE^(@))/(dT)) for a cell are 2V and -5xx10^(-4) Vk^(-1) at 300K respectively . The cell reaction is Zn(s)+ Cu^(2) (aq)+ Cu(S) . The standard reaction enthalpy Delta_(r) H^(@) at 300 K KJmol^(-1) is : ([use R = 8 JK^(-1)mol^(-1) and F = 96000Cmol^(-1)])