Question
Please can you give the "observation" of the production of magnesium sulphate from the reaction of Mg + H2SO4 ...Also write the net ionic equation for the following with indication of their states..
Answers
GPT-4o mini
When magnesium (Mg) reacts with sulfuric acid (H₂SO₄), magnesium sulfate (MgSO₄) and hydrogen gas (H₂) are produced. The balanced chemical equation for the reaction is:
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow \text{MgSO}_4 \text{(aq)} + \text{H}_2 \text{(g)} \]
### Observation:
- **Bubbling/Fizzing**: The reaction will produce bubbles of hydrogen gas, which can be observed as fizzing or effervescence.
- **Temperature Change**: The reaction is exothermic, meaning it may feel warmer as the reaction proceeds.
- **Dissolution of Magnesium**: The magnesium metal will gradually dissolve in the acid, leading to the formation of magnesium sulfate in solution.
### Net Ionic Equation:
1. **Complete Ionic Equation**:
When H₂SO₄ is dissolved in water, it dissociates completely into its ions:
\[ \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow 2 \text{H}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \]
Therefore, the complete ionic equation for the reaction can be written as:
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} + \text{H}_2 \text{(g)} \]
2. **Net Ionic Equation**:
To derive the net ionic equation, we remove the spectator ions (in this case, sulfate ions \(\text{SO}_4^{2-}\), as they appear on both sides of the equation):
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{H}_2 \text{(g)} \]
### Summary:
- **Balanced Overall Equation**:
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow \text{MgSO}_4 \text{(aq)} + \text{H}_2 \text{(g)} \]
- **Net Ionic Equation**:
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{H}_2 \text{(g)} \]
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow \text{MgSO}_4 \text{(aq)} + \text{H}_2 \text{(g)} \]
### Observation:
- **Bubbling/Fizzing**: The reaction will produce bubbles of hydrogen gas, which can be observed as fizzing or effervescence.
- **Temperature Change**: The reaction is exothermic, meaning it may feel warmer as the reaction proceeds.
- **Dissolution of Magnesium**: The magnesium metal will gradually dissolve in the acid, leading to the formation of magnesium sulfate in solution.
### Net Ionic Equation:
1. **Complete Ionic Equation**:
When H₂SO₄ is dissolved in water, it dissociates completely into its ions:
\[ \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow 2 \text{H}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \]
Therefore, the complete ionic equation for the reaction can be written as:
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{SO}_4^{2-} \text{(aq)} + \text{H}_2 \text{(g)} \]
2. **Net Ionic Equation**:
To derive the net ionic equation, we remove the spectator ions (in this case, sulfate ions \(\text{SO}_4^{2-}\), as they appear on both sides of the equation):
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{H}_2 \text{(g)} \]
### Summary:
- **Balanced Overall Equation**:
\[ \text{Mg (s)} + \text{H}_2\text{SO}_4 \text{(aq)} \rightarrow \text{MgSO}_4 \text{(aq)} + \text{H}_2 \text{(g)} \]
- **Net Ionic Equation**:
\[ \text{Mg (s)} + 2\text{H}^+ \text{(aq)} \rightarrow \text{Mg}^{2+} \text{(aq)} + \text{H}_2 \text{(g)} \]