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

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

Accepted Answer

{ "quality": "clear", "question_count": 1, "skills_matched": [ "step_cot", "multiple_choice_formatter", "explain_then_answer", "quick" ], "needs_drawing": false, "concepts_used": [ "Oxidation State Rules", "Oxidation Number Calculation", "Redox Identification", "Oxidized and Reduced Species" ], "new_concepts": [], "current_concepts": [ "Oxidation State Rules", "Oxidation Number Calculation", "Redox Identification", "Oxidized and Reduced Species", "Reducing Agent", "Oxidizing Agent" ] } ## 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 $$ \begin{aligned} &\text{Reducing agent (undergoes oxidation): } \text{Calcium (Ca)} \ &\text{Oxidizing agent (undergoes reduction): } \text{Magnesium ion } (\text{Mg}^{2+} \text{ in } \text{MgI}_2) \end{aligned} $$

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

Iodide is the reducing agent and calcium in the oxidizing agent

{ "subject": "Natural Science", "question_type": "Multiple Choice", "knowledge_point": [ "Natural Science", "Chemistry", "Redox Reactions" ] }

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QUESTION IMAGE

Question

Explanation:

Assign oxidation states to all elements

Identify oxidized and reduced species

Determine reducing and oxidizing agents

Answer: