Complete the chemical reaction.
`Mg_((s))+H_(2)SO_(4(aq))to?`

Options

A. `MgSO_(3)+H_(2)O`
B. `MgSO+H_(2)O+O_(2)`
C. `MgSO_(4)+H_(2)`
D. No reaction

Explanation

To complete the chemical reaction between magnesium (Mg) and sulfuric acid (H₂SO₄), we will follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are magnesium (Mg) in solid form and sulfuric acid (H₂SO₄) in aqueous form.

### Step 2: Determine the Type of Reaction
This is a displacement reaction, where a more reactive metal (magnesium) displaces hydrogen from sulfuric acid.

### Step 3: Write the Displacement Reaction
Since magnesium is more reactive than hydrogen, it will displace the hydrogen ions from sulfuric acid. The reaction can be written as:
\[ \text{Mg}_{(s)} + \text{H}_2\text{SO}_4_{(aq)} \rightarrow \text{MgSO}_4_{(aq)} + \text{H}_2_{(g)} \]

### Step 4: Identify the Products
The products of this reaction are magnesium sulfate (MgSO₄) in aqueous form and hydrogen gas (H₂).

### Final Balanced Equation
The complete balanced chemical equation for the reaction is:
\[ \text{Mg}_{(s)} + \text{H}_2\text{SO}_4_{(aq)} \rightarrow \text{MgSO}_4_{(aq)} + \text{H}_2_{(g)} \]

### Summary of Products
- Magnesium sulfate (MgSO₄) is formed in solution.
- Hydrogen gas (H₂) is released.

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