For a reaction: `X rarr Y+Z`
Absolute entropies are `X="120 J K"^(-1)"mol"^(-1),`
`Y="213.8 J K"^(-1)"mol"^(-1) and Z="197.9 J K"^(-1)"mol"^(-1)`.
What will be the entropy change at 298 K and 1 atm?

The value of DeltaH and DeltaS for two reactions are given below : Reaction A : DeltaH = -10.5 xx 10^(3) J "mol"^(-1) DeltaS = + 31 J K^(-1) "mol"^(-1) Reaction B : DeltaH = -11.7 xx 10^(3) J "mol"^(-1) DeltaS = -105 J K^(-1) "mol"^(-1) Decide whether these reactions are spontaneous or not at 298 K.

For a reaction, X + Y rarr Z there is no entropy charge. Enthaply change for the reaction is 100J mol^(-1) . Delta G is

Calculate the entropy changes for the following reactions : (i) 2CO(g) + O_(2)(g) to 2CO_(2)(g) (ii) 2H_(2)(g) + O_(2)(g) to 2H_(2)O(l) Entropies of different compounds are : CO(g) = 197.6 J K^(-1) "mol"^(-1), O_(2)(g) = 205.03 J K^(-1) "mol"^(-1) CO_(2)(g) = 213.6 JK^(-1) "mol"^(-1), H_(2)(g) = 130.6 J K^(-1) "mol"^(-1) H__(2)O(l) = 69.96 J K^(-1) "mol"^(-1)

The entropy change for eaction at 300 K is 120 Jk^(-1) mol^(-1) . What is the enthalpy change for the reaction ?

For a reaction at 25^(@)C , enthalpy and entropy change are -11.7xx10^(3)J" "mol^(-1) and -150"J "mol^(-1)K^(-1) respectively. What is the Gibbs free energy?

Calculate the entropy change for the following reaction H_(2)(g) +CI_(2)(g) rarr 2HCI (g) at 298 K Given S^(Theta)H_(2) = 131 J K^(-1) mol^(-1), S^(Theta)CI_(2) = 233 J K^(-1) mol^(-1) , and S^(Theta) HCI = 187 J K^(-1) mol^(-1)

Calculate the entropy change for the following reaction H_(2)(g) +CI_(2)(g) rarr 2HCI (g) at 298 K Given S^(Theta)H_(2) = 131 J K^(-1) mol^(-1), S^(Theta)CI_(2) = 233 J K^(-1) mol^(-1) , and S^(Theta) HCI = 187 J K^(-1) mol^(-1)

Calculate the entropy change for the following reaction H_(2)(g) +CI_(2)(g) rarr 2HCI (g) at 298 K Given S^(Theta)H_(2) = 131 J K^(-1) mol^(-1), S^(Theta)CI_(2) = 233 J K^(-1) mol^(-1) , and S^(Theta) HCI = 187 J K^(-1) mol^(-1)