Question

question 9

consider the following chemical reaction:

\\(\text{ca (s)} + \text{mgi}_2\text{ (aq)} \
ightarrow \text{mg (s)} + \text{cai}_2\text{ (aq)}\\)

what is the reducing agent and what is the oxidizing agent?

both magnesium and calcium are reducing agents
calcium is the reducing agent and magnesium is the oxidizing agent
this reaction would not take place since the activity of magnesium is higher than that of calcium
magnesium is the reducing agent and calcium is the oxidizing agent
lodide is the reducing agent and calcium in the oxidizing agent

Explanation:

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"Oxidation Number Calculation",
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"Oxidation Number Calculation",
"Redox Identification",
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"Oxidizing Agent"
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</pre_analysis>

<reasoning>

Assign oxidation states to all elements

\[

$$\begin{aligned} &\text{Reactants:} \\ &\text{Ca}(s): 0 \\ &\text{Mg}^{2+} \text{ in } \text{MgI}_2(aq): +2 \\ &\text{I}^- \text{ in } \text{MgI}_2(aq): -1 \\ &\text{Products:} \\ &\text{Mg}(s): 0 \\ &\text{Ca}^{2+} \text{ in } \text{CaI}_2(aq): +2 \\ &\text{I}^- \text{ in } \text{CaI}_2(aq): -1 \end{aligned}$$

\]

Identify oxidized and reduced species

\[

$$\begin{aligned} &\text{Calcium (Ca): } 0 ightarrow +2 \quad (\text{Oxidized}) \\ &\text{Magnesium (Mg): } +2 ightarrow 0 \quad (\text{Reduced}) \end{aligned}$$

\]

Determine reducing and oxidizing agents

\[

$$\begin{aligned} &\text{Reducing agent (undergoes oxidation): } \text{Calcium (Ca)} \\ &\text{Oxidizing agent (undergoes reduction): } \text{Magnesium ion } (\text{Mg}^{2+} \text{ in } \text{MgI}_2) \end{aligned}$$

\]
</reasoning>

<answer>
<mcq-option>Both magnesium and calcium are reducing agents</mcq-option>
<mcq-correct>Calcium is the reducing agent and magnesium is the oxidizing agent</mcq-correct>
<mcq-option>This reaction would not take place since the activity of magnesium is higher than that of calcium</mcq-option>
<mcq-option>Magnesium is the reducing agent and calcium is the oxidizing agent</mcq-option>
<mcq-option>Iodide is the reducing agent and calcium in the oxidizing agent</mcq-option>
</answer>

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"Redox Reactions"
]
}
</post_analysis>

Answer:

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<reasoning>

Assign oxidation states to all elements

\[

$$\begin{aligned} &\text{Reactants:} \\ &\text{Ca}(s): 0 \\ &\text{Mg}^{2+} \text{ in } \text{MgI}_2(aq): +2 \\ &\text{I}^- \text{ in } \text{MgI}_2(aq): -1 \\ &\text{Products:} \\ &\text{Mg}(s): 0 \\ &\text{Ca}^{2+} \text{ in } \text{CaI}_2(aq): +2 \\ &\text{I}^- \text{ in } \text{CaI}_2(aq): -1 \end{aligned}$$

\]

Identify oxidized and reduced species

\[

$$\begin{aligned} &\text{Calcium (Ca): } 0 ightarrow +2 \quad (\text{Oxidized}) \\ &\text{Magnesium (Mg): } +2 ightarrow 0 \quad (\text{Reduced}) \end{aligned}$$

\]

Determine reducing and oxidizing agents

\[

$$\begin{aligned} &\text{Reducing agent (undergoes oxidation): } \text{Calcium (Ca)} \\ &\text{Oxidizing agent (undergoes reduction): } \text{Magnesium ion } (\text{Mg}^{2+} \text{ in } \text{MgI}_2) \end{aligned}$$

\]
</reasoning>

<answer>
<mcq-option>Both magnesium and calcium are reducing agents</mcq-option>
<mcq-correct>Calcium is the reducing agent and magnesium is the oxidizing agent</mcq-correct>
<mcq-option>This reaction would not take place since the activity of magnesium is higher than that of calcium</mcq-option>
<mcq-option>Magnesium is the reducing agent and calcium is the oxidizing agent</mcq-option>
<mcq-option>Iodide is the reducing agent and calcium in the oxidizing agent</mcq-option>
</answer>

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