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Question 13 of 31

What is the product of the unbalanced equation below?
[tex]\[ \text{Ca (s)} + \text{O}_2\text{(g)} \rightarrow \][/tex]

A. [tex]\(\text{CaO}_2\text{(s)}\)[/tex]
B. [tex]\(2 \text{Ca (s)} + \text{O}_2\text{(g)}\)[/tex]
C. [tex]\(\text{CaO (s)}\)[/tex]
D. [tex]\(\text{Ca}_2\text{O (s)}\)[/tex]

Sagot :

GinnyAnswer
In examining the reaction between calcium (Ca) in its solid form and oxygen (O₂) in its gaseous form, we must determine what product is formed when these elements react.

1. Identify the Reactants: The reactants given are:
- Calcium (Ca) in solid form.
- Oxygen (O₂) in gaseous form.

2. Understand the Nature of the Reaction:
- Calcium is a metal.
- Oxygen is a diatomic gas that usually reacts with metals to form oxides.

3. Predict the Product:
- Typically, when a metal reacts with oxygen, it forms a metal oxide.

4. Consider the Possible Products:
- Option A: [tex]\( CaO_2(s) \)[/tex] : This implies calcium peroxide, which is not a common result of direct reaction between calcium and oxygen.
- Option B: [tex]\( 2 Ca(s) + O_2(g) \)[/tex] : This represents the reactants but not the product.
- Option C: [tex]\( CaO(s) \)[/tex] : This is calcium oxide, a common product of the reaction between calcium and oxygen.
- Option D: [tex]\( Ca_2O(s) \)[/tex] : This does not align with typical stoichiometry for calcium oxide.

5. Choose the Correct Product:
- The typical product when calcium reacts with oxygen is calcium oxide, with the formula [tex]\( CaO \)[/tex].

Therefore, the answer is:
[tex]\[ \boxed{CaO(s)} \][/tex]
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