Question
Please can you do the net ionic equation for the reaction of magnesium metal pieces reacted with H2SO4, and also give the observation of the reaction?
Answers
GPT-4o mini
When magnesium metal (Mg) reacts with sulfuric acid (H₂SO₄), the reaction produces magnesium sulfate (MgSO₄), hydrogen gas (H₂), and heat. The overall balanced chemical equation for this reaction can be written as follows:
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 (aq) \rightarrow \text{MgSO}_4 (aq) + \text{H}_2 (g) \]
To derive the net ionic equation, we need to consider the dissociation of the strong acid in solution. Sulfuric acid dissociates into hydrogen ions (H⁺) and sulfate ions (SO₄²⁻). The magnesium sulfate that forms is soluble in water and dissociates into magnesium ions (Mg²⁺) and sulfate ions (SO₄²⁻).
1. The complete ionic equation is:
\[ \text{Mg (s)} + 2\text{H}^+ (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{Mg}^{2+} (aq) + \text{SO}_4^{2-} (aq) + \text{H}_2 (g) \]
2. In this equation, the sulfate ions (SO₄²⁻) are present on both sides and can be cancelled out, leading to the net ionic equation:
**Net Ionic Equation:**
\[ \text{Mg (s)} + 2\text{H}^+ (aq) \rightarrow \text{Mg}^{2+} (aq) + \text{H}_2 (g) \]
### Observations of the Reaction:
1. **Bubbles of Hydrogen Gas**: As magnesium reacts with sulfuric acid, bubbles of hydrogen gas will be observed rising from the surface of the magnesium.
2. **Heat Evolution**: The reaction is exothermic, so you may also feel heat being released during the reaction.
3. **Dissolution of Magnesium**: The magnesium metal will gradually dissolve as it reacts with the acid.
Overall, the reaction shows clear evidence of a chemical change as magnesium is converted to magnesium ions, and hydrogen gas is produced.
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 (aq) \rightarrow \text{MgSO}_4 (aq) + \text{H}_2 (g) \]
To derive the net ionic equation, we need to consider the dissociation of the strong acid in solution. Sulfuric acid dissociates into hydrogen ions (H⁺) and sulfate ions (SO₄²⁻). The magnesium sulfate that forms is soluble in water and dissociates into magnesium ions (Mg²⁺) and sulfate ions (SO₄²⁻).
1. The complete ionic equation is:
\[ \text{Mg (s)} + 2\text{H}^+ (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{Mg}^{2+} (aq) + \text{SO}_4^{2-} (aq) + \text{H}_2 (g) \]
2. In this equation, the sulfate ions (SO₄²⁻) are present on both sides and can be cancelled out, leading to the net ionic equation:
**Net Ionic Equation:**
\[ \text{Mg (s)} + 2\text{H}^+ (aq) \rightarrow \text{Mg}^{2+} (aq) + \text{H}_2 (g) \]
### Observations of the Reaction:
1. **Bubbles of Hydrogen Gas**: As magnesium reacts with sulfuric acid, bubbles of hydrogen gas will be observed rising from the surface of the magnesium.
2. **Heat Evolution**: The reaction is exothermic, so you may also feel heat being released during the reaction.
3. **Dissolution of Magnesium**: The magnesium metal will gradually dissolve as it reacts with the acid.
Overall, the reaction shows clear evidence of a chemical change as magnesium is converted to magnesium ions, and hydrogen gas is produced.