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Consider the reaction 2NO(g) + O(2)(g)...

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`

A

Yes , Spontaneous

B

No, the reaction is Non-spontaneous

C

Equilibrium

D

Cannot predict

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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.

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.

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) .

Will the reaction, I_(2)(s) +H_(2)S(g) rarr 2HI(g) +S(s) proceed spontaneously in the forward direction of 298K Delta_(f)G^(Theta)HI(g) = 1.8 kJ mol^(-1), Delta_(f)G^(Theta)H_(2)S(g) = 33.8 kJ mol^(-1) ?

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"

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