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For the reaction N(2)(g) + 3 H(2) righ...

For the reaction
`N_(2)(g) + 3 H_(2) rightarrow 2NH_(3)(g) `
`Delta H = -85.4 kJ and Delta S = - 188.3 Jk^(-1)`
Calculate the temperature at which Gibs energy change(`Delta G`) is equal to zero. Predict the nature of the reaction at this temperature and above it.

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To solve the problem, we need to calculate the temperature at which the Gibbs energy change (ΔG) is equal to zero for the given reaction: \[ N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) \] Given: - ΔH = -85.4 kJ - ΔS = -188.3 J/K ...
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