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For the reaction `: 2NO(g) + O_(2)(g) rarr 2NO_(2)(g)`, the enthalpy and entropy changes are - 113.0 kJ `mol^(-1)` and `-145 JK^(-1) mol^(-1)` respectively. Find the temperature below which this reaction is spontaneous.

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Correct Answer - 779.3K
`DeltaG = DeltaH - T DeltaS`. When reaction is in equilibrium , `DeltaG =0.` `:. T = (DeltaH)/(DeltaS) = ( -113000J mol^(-1))/( - 145 JK^(-1)mol^(-1)) = 779.3K`.
For reaction to be spontaneous , `Delta G ` should be -ve which can be so if temperature is below ` 779.3K`

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