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

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)`.

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To solve the problem, we need to calculate the standard Gibbs energy change (ΔG°) for the reaction: \[ 2NO(g) + O_2(g) \rightarrow 2NO_2(g) \] We will use the given standard Gibbs free energies of formation (ΔG°f) for the reactants and products: - ΔG°f (NO) = 86.69 kJ/mol - ΔG°f (NO₂) = 51.84 kJ/mol ...
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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) , 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

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