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The problem asks to calculate the equilibrium concentration of oxygen (\(\text{O}_2\)) in the given chemical reaction:

\[
4\text{NH}_3 (g) + 7\text{O}_2 (g) \rightleftharpoons 2\text{N}_2\text{O}_4 (g) + 6\text{H}_2\text{O} (g)
\]

### Known values:
- Initial concentration of \(\text{NH}_3\) and \(\text{O}_2\): \([\text{NH}_3] = [\text{O}_2] = 3.60\,M\)
- At equilibrium: \( [\text{N}_2\text{O}_4] = 0.60\,M \)

### Step-by-step solution:

1. **Write the balanced equation**:

   \[
   4\text{NH}_3 + 7\text{O}_2 \rightleftharpoons 2\text{N}_2\text{O}_4 + 6\text{H}_2\text{O}
   \]

2. **Set up the ICE table** (Initial, Change, Equilibrium):

   | Species         | \([\text{NH}_3]\) | \([\text{O}_2]\) | \([\text{N}_2\text{O}_4]\) | \([\text{

A study of the system, 4NH3(g) + 7O2(g) ⇌ 2N2O4(g) + 6H2O(g), was carried out. A system was prepared with [NH3] = [O2] = 3.60 M as the only components initially. At equilibrium, [N2O4] is 0.60 M. Calculate the equilibrium concentration of O2.

This problem focuses on determining the equilibrium concentration of O2 in the reaction between ammonia (NH3) and oxygen (O2). It involves setting up an ICE table and using stoichiometric ratios to find the unknown concentration. Suitable for advanced chemistry students.

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