For a reaction `A+2BtoC+D`, if `DeltaH=-25kcal`, `T=300 K` and `DeltaS=90 cal`, then the reaction is

DeltaG for a reaction at 300 K is -16 kcal and DeltaH is -10 kcal . The entropy of the reaction is

For the reaction at 298 K A(g) + B(g) hArr C(g) + D(g) If DeltaH^(@) =29.8 Kcal and DeltaS^(@)=0.1 Kcal K^(-1) then calculate reaction constant (k)

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 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) )

For the reaction at 298 K A(g) + B(g) hArr C(g) + D(g) If DeltaH^(@) =-29.8 Kcal and DeltaS^(@) Kcal K^(-1) then calculate reaction constant (k)

For the reaction at 25^(@)C,X_(2)O_(4(l))to2XO_(2(g)),DeltaH=2.1kcal and DeltaS=20" cal "K^(-1) . The reaction would be

Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (DeltaG)_(PT) = DeltaH - T DeltaS The magnitude of DeltaH does not change much with the change in temperature but the enrgy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. For the reaction at 25^(2)C, X_(2)O_(4)(l) rarr 2XO_(2) DeltaH = 2.0 kcal and DeltaS = 20 cal K^(-1) . the reaction would be

Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (DeltaG)_(PT) = DeltaH - T DeltaS The magnitude of DeltaH does not change much with the change in temperature but the energy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. For the reaction at 25^(0)C, X_(2)O_(4)(l) rarr 2XO_(2) DeltaH = 2.0 kcal and DeltaS = 20 cal K^(-1) . the reaction would be