The enthalpy change (`DeltaH`) for the reaction
`Ag_2O(s) hArr 2Ag(s) + 1/2 O_2(g)`
is `30.54 kJ mol^(-1)` and entropy change `(DeltaS)` is `0.06 kJ K^(-1) mol^(-1)` at 1 atm. Calculate the temperature at which `DeltaG` is equal to zero. Also predict the direction of reaction at a temperature below the calculated temperature.

Explanation

To solve the problem, we need to calculate the temperature at which the Gibbs free energy change (ΔG) for the reaction is equal to zero. We will use the relationship between ΔG, ΔH, and ΔS, which is given by the equation:

\[ \Delta G = \Delta H - T \Delta S \]

### Step 1: Set ΔG to zero
Since we want to find the temperature at which ΔG = 0, we can set up the equation:
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