Caculate `DeltaG(kJ//"mole") "for the reaction at 300K"`
`N_(2)(g)+O_(2)(g)Leftrightarrow 2NO(g)`
at constant where partical pressure of `N_(2), O_(2)` and `NO are 10^(-1)"bar", 10^(-3)"bar"`. `DeltaH_(f)^(@)NO(g) at 300K =90.5kJ//"mole"and DeltaS_(f)^(@),NO(g) at 300K =12.5J//K"mole"and DeltaS_(f)^(@)NO(g)at 300k=12.5J//K"mole" "` `[2.303xxRxx300=5750J//"mole"]`

Calculate DeltaG_(reaction) ("kJ"//"mol") for the given reaction at 300 K A_(2)(g)+B_(2)(g)hArr2Ab(g) and at particle pressure of 10^(-2) bar and 10^(-4) Given : Delta H_(f)^(@) AB =180 kJ//mol," "DeltaH_(f)^(@) A_(2)=60 kJ//mol Delta H_(f)^(@) B_(2) = 29.5 kJ//mol," "DeltaS_(f)^(@) AB=210 J//K-mol Delta S_(f)^(@) A_(2) = 190 kJ//mol," "DeltaS_(f)^(@) B_(2)=205 J//K-mol Use : 2.303 Rxx300=5750 "J"//"mole"

Calculate the DeltaG^0 for the reaction N_2(g) + O_2(g) * 2NO(g) Given DeltaH^0 =180.5 K.J , and DeltaS^0 = 15 J at 25^@C .

Determine the entropy change for the reaction 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l) at 300K . If standard entropies of H_(2)(g),O_(2)(g) and H_(2)O(l) are 12.6, 201.20 and 68.0 J K^(-1) "mole"^(-1) respectively.

Determine the entropy change for the reaction 2H_(2)(g) +O_(2)(g) rarr 2H_(2)O(l) at 300K . If standard entropies of H_(2)(g),O_(2)(g) and H_(2)O(l) are 12.6, 201.20 and 68.0 J K^(-1) "mole"^(-1) respectively.

For the f reaction at 300K A(g)+B(g) to C(g) DeltaU = - 3.0 k cal" "," "DeltaS = - 10.0 cal //K Value of the DeltaG is

For the reaction, X_(2)O_(4)(l)to2XO_(2)(g),DeltaU=2.1 kcal, DeltaS=20cal*K^(-1) at 300K, hence, DeltaG is -

For the reaction, X_(2)O_(4)(l)rarr2XO_(2)(g) , DeltaE=3.1Kcal , DeltaS=30cal//K at 300K . Hence DeltaG is