For the reaction `N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g)`,
Calculate `Delta_(r)S^(o)` (in `J/(mol-K)`) at `300K`.
Given: `(Delta H_(f)^(o))_(NH_(3).300K)=-46(kJ)/(mol)`
`(Delta G_(f)^(o))_(NH_(3).300K)=-16(kJ)/(mol)`

Given N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g),Delta_(r)H^(Ө)= -92.4 kJ mol^(-1) What is the standard enthalpy of formation of NH_(3) gas?

Given N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g),Delta_(r)H^(Ө)= -92.4 kJ mol^(-1) What is the standard enthalpy of formation of NH_(3) gas?

For the reaction : C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(g) if Delta U^(@)= -1373 kJ mol^(-1) at 298 K . Calculate Delta H^(@)

Determine the enthalpy of formation of B_(2)H_(6) (g) in kJ/mol of the following reaction : B_(2)H_(6)(g)+3O_(2)(g)rarrB_(2)O_(3)(s)+3H_(2)O(g) , Given : Delta_(r )H^(@)=-1941 " kJ"//"mol", " "DeltaH_(f)^(@)(B_(2)O_(3),s)=-1273" kJ"//"mol," DeltaH_(f)^(@)(H_(2)O,g)=-241.8 " kJ"//"mol"

For the reaction X_(2)O_(4(l)) rarr 2XO_(2(g)), Delta U= 2.1 "kcal", Delta S= 20 "cal " K^(-1) at 300K, Hence Delta G is

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

For the reaction N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) , DeltaH = -93.6 KJ mol^(-1) the formation of NH_(3) is expected to increase at :

For the reaction, X_(2)O_(4)(l)rarr2XO_(2)(g),DeltaE=2.1Kcal , DeltaS=20cal//K at 300K . Hence DeltaG is

Consider the reaction: 4NH_(3)(g) +5O_(2)(g) rarr 4NO(g) +6H_(2)O(l) DeltaG^(Theta) =- 1010.5 kJ Calculate Delta_(f)G^(Theta) [NO(g)] if Delta_(f)G^(Theta) (NH_(3)) = -16.6 kJ mol^(-1) and Delta_(f)G^(Theta) [H_(2)O(l)] =- 237.2 kJ mol^(-1) .

For the reaction: CO(g) +H_(2)O(g) hArr CO_(2)(g) +H_(2)(g) (Delta_(r)H)_(300K) = - 41.2 kJ mol^(-1) (Delta_(r)H)_(1200K) =- 33.0 kJ mol^(-1) (Delta_(r)S)_(300K) = - 4.2 xx 10^(-2) kJ mol^(-1) (Delta_(r)S)_(1200K) =- 3.0 xx10^(-2) kJ mol^(-1) Predict the direction of spontaneity of the reaction at 300K and 1200K . also calculated log_(10)K_(p) at 300K and 1200K .