For the question(s) that follow, consider the following equation. \( 2 \mathrm{Mg}+\mathrm{O} 2 \rightarrow 2 \mathrm{MgO} \) Part A The number of moles of oxygen gas needed to react with 4.0 moles of Mg is 1.0 mole. 2.0 moles. 3.0 moles. 6.0 moles. Submit Request Answer Part R

The balanced equation \( 2 \mathrm{Mg} + \mathrm{O}_2 \rightarrow 2 \mathrm{MgO} \) shows that 2 moles of magnesium (Mg) react with 1 mole of oxygen gas (\( \mathrm{O}_2 \)). This means for every 2 moles of Mg, only 1 mole of \( \mathrm{O}_2 \) is required. If you have 4.0 moles of Mg, you can apply a simple ratio: for 4 moles of Mg, you'd need \( \frac{4}{2} = 2 \) moles of \( \mathrm{O}_2 \). So the answer is 2.0 moles. Next, beyond just the numbers, it's fascinating to think about how this reaction exemplifies the principles of stoichiometry—like a dance between elements where one helps another attain stability! When metals like magnesium meet diatomic gases like oxygen, they form stable compounds, shedding light on nature's way of achieving balance and harmony in chemical reactions. It's not just chemistry; it's a beautiful interplay!