` 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 :

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.

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 ?

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 .

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)])

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 300K . If the emf of the cell is zero, the DeltaS^(@) (in JK^(-1mol^(-1)) of the cell reaction per mole of B formed at 300 K is _________. (Given ln (2)= 0.7, R (universal gas constant ) = 8.3JK^(-1)mol^(-1) . H, S and G are enthalpy , entropy and gibbs energy, respectively).

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.)

The standard enthalpy and entropy changes for the reaction in equilibrium for the forward direction are given below: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) DeltaH^(Theta)underset(300K). =- 41.16 kJ mol^(-1) DeltaS^(Theta)underset(300K). =- 4.24 xx 10^(-2) kJ mol^(-1) DeltaH^(Theta)underset(1200K). =- 32.93 kJ mol^(-1) DeltaH^(Theta)underset(1200K). =- 2.96 xx 10^(-2) kJ mol^(-1) Calculate K_(p) at each temperature and predict the direction of reaction at 300K and 1200k , when P_(CO) = P_(CO_(2)) =P_(H_(2)) = P_(H_(2)O) =1 atm at initial state.