Question
Write the total ionic and net ionic equation for the following. Consider the balance equation as well as stage.
C. Fe (s) +HCl (aq) = FeCl2 (aq) +H2O (g)
C. Fe (s) +HCl (aq) = FeCl2 (aq) +H2O (g)
Answers
GPT-4o mini
Let's start with the balanced molecular equation for the reaction between iron (Fe) and hydrochloric acid (HCl):
\[
\text{Fe (s)} + 2 \text{HCl (aq)} \rightarrow \text{FeCl}_2 \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Total Ionic Equation
To write the total ionic equation, we need to dissociate all the strong electrolytes (soluble ionic compounds and acids) into their respective ions. HCl is a strong acid and will dissociate fully in aqueous solution, while FeCl\(_2\) is a soluble salt that will also dissociate into its ions. However, solid metals and gases remain in their molecular forms:
1. Dissociated HCl: \(2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)}\)
2. Dissociated FeCl\(_2\): \(\text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)}\)
Putting this all together, we have:
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Cancel Common Ions
Now we can simplify this to get the net ionic equation by removing the spectator ions. In this reaction, Chloride ions (\( \text{Cl}^- \)) appear on both sides and can be canceled out:
### Net Ionic Equation
After canceling the spectator ions:
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Summary
**Total Ionic Equation:**
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
**Net Ionic Equation:**
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
\[
\text{Fe (s)} + 2 \text{HCl (aq)} \rightarrow \text{FeCl}_2 \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Total Ionic Equation
To write the total ionic equation, we need to dissociate all the strong electrolytes (soluble ionic compounds and acids) into their respective ions. HCl is a strong acid and will dissociate fully in aqueous solution, while FeCl\(_2\) is a soluble salt that will also dissociate into its ions. However, solid metals and gases remain in their molecular forms:
1. Dissociated HCl: \(2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)}\)
2. Dissociated FeCl\(_2\): \(\text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)}\)
Putting this all together, we have:
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Cancel Common Ions
Now we can simplify this to get the net ionic equation by removing the spectator ions. In this reaction, Chloride ions (\( \text{Cl}^- \)) appear on both sides and can be canceled out:
### Net Ionic Equation
After canceling the spectator ions:
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
### Summary
**Total Ionic Equation:**
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + 2 \text{Cl}^- \text{ (aq)} + \text{H}_2 \text{ (g)}
\]
**Net Ionic Equation:**
\[
\text{Fe (s)} + 2 \text{H}^+ \text{ (aq)} \rightarrow \text{Fe}^{2+} \text{ (aq)} + \text{H}_2 \text{ (g)}
\]