Find DeltaG `(J//"mol")` for the reaction at `300 kPa` and `27^(@)C` when all gases are in stoichimetric ratio of moles. `N_(2)O_(4)(g)rarr2NO_(2)(g)` `[ln 2=0.7]`
Given : `DeltaG_(f)^(@)(N_(2)O_(4))=100"kJ/mol"`
`DeltaG_(f)^(@)(NO_(2))=50"kJ/mol"`
`R=8"J/mol"-K`

Find out InK_(eq) for the formation of NO_(2) from NO and O_(2) at 298 K NO_(g)+(1)/(2)O_(2)hArrNO_(2)g Given: DeltaG_(f)^(@)(NO_(2))=52.0KJ//mol e Delta_(f)^(@)(NO)=87.0KJ//mol e Delta_(f)^(@)(O_(2))=0KJ//mol e

Find out InK_(eq) for the formation of NO_(2) from NO and O_(2) at 298 K NO_(g)+(1)/(2)O_(2)hArrNO_(2)g Given: DeltaG_(f)^(@)(NO_(2))=52.0KJ//mol e Delta_(f)^(@)(NO)=87.0KJ//mol e Delta_(f)^(@)(O_(2))=0KJ//mol e

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"

For the reaction at 300 K, N_2O_4(g)hArr2NO_2(g) , the value of DeltaG when concentration of each species is 5 mol/litre, will be (Given: ( DeltaG_(fN_2O_4)^o ) = 120 kJ/mol and ( DeltaG_(fNO_2)^o ) = 70 kJ/mol)

Calculate (1) DeltaG^(0) and (2) The equilibrium constant for the formation of NO_(2) from NO and O_(2) at 298K. NO(g)+1//2O_(2)(g)hArr NO_(2)(g) where Delta_(f)DeltaG^(0)(NO_(2))=52.0kJ//mol , Delta_(f)G^(0)(NO)=87.0kJ//mol,Delta_(f)G^(0)(O_(2))=0kJ//mol

The minimum voltage required to electrolyse alumina in the Hall-Heroul process is [Given, DeltaG^(@)_(f)(A1_(2)O_(3)) =- 1520kJ//mol and DeltaG^(@)_(f)(CO_(2)) = 394kJ//mol]

The minimum voltage required to electrolyse alumina in the Hall-Heroul process is [Given, DeltaG^(@)_(f)(A1_(2)O_(3)) =- 1520kJ//mol and DeltaG^(@)_(f)(CO_(2)) = 394kJ//mol]

Calculate a) DeltaG^(@) and b) the equilibrium constant for the formation of NO_(2) from NO and O_(2) at 298K NO(g)+1//2O_(2)(g)hArrNO_(2)(g) where Delta_(f)G^(oplus)(NO_(2))=52.0kJ//mol Delta_(f)G^(oplus)(NO)=87.0kJ//mol Delta_(f)G^(oplus)(O_(2))=0kJ//mol

Consider the reaction 2NO(g) + O_(2)(g) rarr 2NO_(2)(g) , Predict whether the reaction is spontaneous at 298 K. Delta_(f) G(NO) = 86.69k J//mol,Delta _(f) G ( NO_(2) = 51.84 kJ//mol