For the reaction,
`2NO_(g) + O_(2)(g) rarr 2NO_(2)(g)`
Calculate `DeltaG` at `700K` when enthalpy and entropy changes are `-113.0 kJ mol^(-1)` and `-145 J K^(-1) mol^(-1)`, respectively.

Explanation

To calculate the Gibbs free energy change (ΔG) for the reaction \(2NO(g) + O_2(g) \rightarrow 2NO_2(g)\) at 700 K, given the enthalpy change (ΔH) and entropy change (ΔS), we can follow these steps:

### Step 1: Write the Gibbs Free Energy Equation
The relationship between Gibbs free energy change, enthalpy change, and entropy change is given by the equation:
\[ \Delta G = \Delta H - T \Delta S \]

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