To calculate the number of grams of magnesium (Mg) required to react completely with 2 moles of hydrochloric acid (HCl), follow these steps:
### Step 1: Write the balanced chemical equation.
The reaction between magnesium and hydrochloric acid can be represented by the balanced chemical equation:
[tex]\[ \text{Mg} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2 \][/tex]
### Step 2: Analyze the stoichiometry of the reaction.
From the balanced equation, we see that:
- 1 mole of Mg reacts with 2 moles of HCl.
Therefore, the mole ratio between Mg and HCl is 1:2.
### Step 3: Determine the moles of magnesium needed.
Given that we have 2 moles of HCl, we can use the stoichiometric ratio to find the moles of Mg required:
[tex]\[ \text{Moles of Mg} = \frac{\text{Moles of HCl}}{2} \][/tex]
[tex]\[ \text{Moles of Mg} = \frac{2 \text{ moles of HCl}}{2} \][/tex]
[tex]\[ \text{Moles of Mg} = 1 \text{ mole} \][/tex]
### Step 4: Calculate the grams of magnesium needed.
The molar mass of magnesium (Mg) is approximately [tex]\( 24.305 \)[/tex] grams per mole. Now, using the moles of Mg calculated in the previous step:
[tex]\[ \text{Mass of Mg} = \text{Moles of Mg} \times \text{Molar mass of Mg} \][/tex]
[tex]\[ \text{Mass of Mg} = 1 \text{ mole} \times 24.305 \text{ grams/mole} \][/tex]
[tex]\[ \text{Mass of Mg} = 24.305 \text{ grams} \][/tex]
Therefore, [tex]\( 24.305 \)[/tex] grams of magnesium are required to react completely with 2 moles of hydrochloric acid.
