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 (A) -25.1kJmol^(-1) (B) +25.1kJmol^(-1) 18.7kJmol^(-1) (c) 0.08367kJ.K^(-1).mol^(-1)

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 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 ?

Given that Bond energy of H_(2) and N_(2) are 400KJmol^(-1) and 240KJmol^(-1) respectively and DeltaH_(f) of NH_(3) is -120KJmol^(-1) calculate the bond energy of N-H bond :-

If for a reaction A(s) rarr 2B(g), deltaU+ 1.2 kcal and deltaS=40 cal K^(-1) at 400K then deltaG for the reaction will be ( R=2 cal mol^(-1)K^(-1)

If EA_1 and EA_2 for oxygen atom -142kJmol"^(-1) and +844kJmol^(-1) . The energy released form 2O+2e^(-)rarr2O^(-) will be

The value of log_(10)K for a reaction A hArr B is (Given: Delta_(f)H_(298K)^(Theta) =- 54.07 kJ mol^(-1) , Delta_(r)S_(298K)^(Theta) =10 JK^(=1) mol^(-1) , and R = 8.314 J K^(-1) mol^(-1)

Standard enthalpy of vapourisation Delta_(vap) H^- for water at 100° C is 56.66 kJmol^(–1) . The internal energy of vapourisation of water at 100°C (in kJmol^(–1) ) is ?

Standard enthalpy of vapourisation Delta_(vap) H^- for water at 100° C is 50.66 kJmol^(–1) . The internal energy of vapourisation of water at 100°C (in kJmol^(–1) ) is ?

Standard enthalpy of vapourisation Delta_(vap) H^- for water at 100° C is 44.66 kJmol^(–1) . The internal energy of vapourisation of water at 100°C (in kJmol^(–1) ) is ?

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 .