`Delta H` and `Delta S` for the reaction, `Ag_(2)O(s)to 2A(s)+(1)/(2)O_(2)(g)`, are 30.56 kJ `mol^(-1)` and 66.0 J `mol^(-1)` respectively. Calculate the temperature at which this reaction will be at equilibrium. Predict whether the forward reaction will be favoured above or below this temperature.

Explanation

To solve the problem, we need to find the temperature at which the reaction \( \text{Ag}_2\text{O}(s) \rightarrow 2\text{Ag}(s) + \frac{1}{2}\text{O}_2(g) \) will be at equilibrium. We are given the values of \( \Delta H \) and \( \Delta S \) for the reaction:

- \( \Delta H = 30.56 \, \text{kJ mol}^{-1} \)
- \( \Delta S = 66.0 \, \text{J mol}^{-1} \)

### Step 1: Convert \( \Delta H \) to Joules
Since \( \Delta S \) is given in Joules, we need to convert \( \Delta H \) from kJ to J.

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