Answer:
[tex]\large \boxed{4.81 \times 10^{-22} \text{ g Mg}}[/tex]
Explanation:
We will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.
Mᵣ: 24.30
Mg + 2H⁺ ⟶ Mg²⁺ + H₂
n/mol: 1.98 × 10⁻²³
1. Calculate the moles of Mg
The molar ratio is 1 mol Mg:1 mol H₂
[tex]\rm \text{Moles of Mg} =1.98 \times 10^{-23} \text{ mol H}_{2} \times \dfrac{\text{1 mol Mg}}{\text{1 mol H}_{2}} = 1.98 \times 10^{-23} \text{ mol Mg}[/tex]
2. Calculate the mass of Mg
[tex]\text{Mass of Mg} = 1.98 \times 10^{-23} \text{ mol Mg} \times \dfrac{\text{24.30 g Mg}}{\text{1 mol Mg}} = \mathbf{4.81 \times 10^{-22}} \textbf{ g Mg}\\\\\text{The mass of Mg reacted is $\large \boxed{\mathbf{4.81 \times 10^{\mathbf{-22}} \textbf{ g Mg}}}$}[/tex]
