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`

At 298 K, K_(p) for the reaction : N_(2)O_(4)(g) iff 2NO_(2)(g) is 0.98. Predict whether the reaction is spontaneous or not.

At 298 K, K_(p) for reaction N_(2)O_(4) (g) hArr 2NO_(2) (g) is 0.98. Predict whether the reaction is spontaneous or not.

Consider the reaction: 2NO(g)+O_(2)(g) rarr 2NO_(2)(g) Calculated the standard Gibbs energy change at 298K and predict whether the reaction is spontaneous or not. Delta_(f)G^(Theta) (NO) = 86.69 kJ mol^(-1), Delta_(f)G^(Theta) (NO_(2)) = 51.84 kJ mol^(-1) .

Consider the reaction: 2NO(g)+O_(2)(g) rarr 2NO_(2)(g) Calculated the standard Gibbs energy change at 298K and predict whther the rection is spontaneous or not. Delta_(f)G^(Theta) (NO) = 86.69 kJ mol^(-1), Delta_(f)G^(Theta) (NO_(2)) = 51.84 kJ mol^(-1) .

Consider the reaction: 2NO(g)+O_(2)(g) rarr 2NO_(2)(g) Calculated the standard Gibbs energy change at 298K and predict whther the rection is spontaneous or not. Delta_(f)G^(Theta) (NO) = 86.69 kJ mol^(-1), Delta_(f)G^(Theta) (NO_(2)) = 51.84 kJ mol^(-1) .

Calculate (a) DeltaG^(Theta) and (b) the equilibrium constant for the formation of NO_(2) from NO and O_(2) at 298 K NO(g) +1//2 O_(2) (g) hArr NO_(2)(g) where Delta_(f) G^(Theta) (NO_(2)) =52 .0 kJ//mol, Delta_(f) G^(Theta) (NO) =87.0 kJ//mol, Delta_(f) G^(Theta) (O_(2)) =0kJ//mol.