Question

question 1 (1 point)
what is the correct balanced net ionic equation for the reaction:
fe(no₃)₂(aq) + ni(s) → fe(s)+ni(no₃)₂(aq)

2fe²⁺(aq) + 3ni(s) → 2fe(s)+3ni²⁺(aq)

3fe²⁺(aq) + 2ni(s) → 3fe(s)+2ni²⁺(aq)

fe²⁺(aq) + ni(s) → fe(s)+ni²⁺(aq)

fe(no₃)₂(aq) + ni(s) → fe(s)+ni(no₃)₂(aq)

2fe(no₃)₂(aq) + 3ni(s) → 2fe(s)+3ni(no₃)₂(aq)

Explanation:

Step1: Identify soluble compounds and ions

First, we recognize that \( \text{Fe(NO}_3\text{)}_2 \) and \( \text{Ni(NO}_3\text{)}_2 \) are soluble ionic compounds. So, they dissociate into ions in aqueous solution:
\( \text{Fe(NO}_3\text{)}_2(\text{aq})
ightarrow \text{Fe}^{2+}(\text{aq}) + 2\text{NO}_3^-(\text{aq}) \)
\( \text{Ni(NO}_3\text{)}_2(\text{aq})
ightarrow \text{Ni}^{2+}(\text{aq}) + 2\text{NO}_3^-(\text{aq}) \)

Step2: Write the total ionic equation

Substitute the dissociated ions into the original reaction:
\( \text{Fe}^{2+}(\text{aq}) + 2\text{NO}_3^-(\text{aq}) + \text{Ni}(\text{s})
ightarrow \text{Fe}(\text{s}) + \text{Ni}^{2+}(\text{aq}) + 2\text{NO}_3^-(\text{aq}) \)

Step3: Cancel spectator ions

The \( \text{NO}_3^- \) ions appear on both sides (spectator ions), so we cancel them:
\( \text{Fe}^{2+}(\text{aq}) + \text{Ni}(\text{s})
ightarrow \text{Fe}(\text{s}) + \text{Ni}^{2+}(\text{aq}) \)

Step4: Check balancing

The number of each atom and the charge are balanced:

• Fe: 1 on left, 1 on right.
• Ni: 1 on left, 1 on right.
• Charge: Left: \( +2 + 0 = +2 \); Right: \( 0 + +2 = +2 \).

Answer:

\( \boldsymbol{\text{Fe}^{2+}(\text{aq}) + \text{Ni}(\text{s})
ightarrow \text{Fe}(\text{s}) + \text{Ni}^{2+}(\text{aq})} \) (corresponding to the option: \( \text{Fe}^{2+}(\text{aq}) + \text{Ni}(\text{s})
ightarrow \text{Fe}(\text{s})+\text{Ni}^{2+}(\text{aq}) \))