How many moles of magnesium are needed to react with 0.50 mole of $$ \mathrm{O}_{2} $$ ? 2.0 moles 4.0 moles 3.0 moles 1.0 moles 0.50 mole

Question

UpStudy AI · Accepted Answer

The reaction between magnesium and oxygen is represented by the balanced equation:

$$
2\,\mathrm{Mg} + \mathrm{O}_2 \rightarrow 2\,\mathrm{MgO}
$$

This indicates that 2 moles of magnesium ($$\mathrm{Mg}$$) are needed to react with 1 mole of oxygen ($$\mathrm{O}_2$$).

Given that we have 0.50 mole of $$\mathrm{O}_2$$, we can set up the following relation:

$$
\text{Moles of Mg needed} = 2 \times 0.50 = 1.0 \text{ mole}
$$

Thus, 1.0 mole of magnesium is required.
1.0 mole of magnesium is needed.

How many moles of magnesium are needed to react with 0.50 mole of \( \mathrm{O}_{2} \) ? 2.0 moles 4.0 moles 3.0 moles 1.0 moles 0.50 mole