Question
Question 15
Balance the following the chemical equation:
_____Mg+_____O2--->_____MgO
Balance the following the chemical equation:
_____Mg+_____O2--->_____MgO
Answers
Answered by
GPT-4o mini
To balance the chemical equation for the reaction between magnesium (Mg) and oxygen (O₂) to form magnesium oxide (MgO), follow these steps:
1. Write the unbalanced equation:
\[
\text{Mg} + \text{O}_2 \rightarrow \text{MgO}
\]
2. Count the number of atoms for each element on both sides of the equation:
- Reactants: 1 Mg, 2 O (from O₂)
- Products: 1 Mg, 1 O (from MgO)
3. To balance the oxygen, you need 2 oxygen atoms in the products. Since there is only 1 oxygen atom in MgO, you will need 2 MgO to balance the oxygen:
\[
\text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}
\]
4. Now, you have 2 magnesium atoms on the product side. You need to add a coefficient of 2 in front of Mg in the reactants:
\[
2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}
\]
Now the equation is balanced:
- Reactants: 2 Mg, 2 O (from O₂)
- Products: 2 Mg, 2 O (from 2 MgO)
The balanced chemical equation is:
\[
\boxed{2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}}
\]
1. Write the unbalanced equation:
\[
\text{Mg} + \text{O}_2 \rightarrow \text{MgO}
\]
2. Count the number of atoms for each element on both sides of the equation:
- Reactants: 1 Mg, 2 O (from O₂)
- Products: 1 Mg, 1 O (from MgO)
3. To balance the oxygen, you need 2 oxygen atoms in the products. Since there is only 1 oxygen atom in MgO, you will need 2 MgO to balance the oxygen:
\[
\text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}
\]
4. Now, you have 2 magnesium atoms on the product side. You need to add a coefficient of 2 in front of Mg in the reactants:
\[
2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}
\]
Now the equation is balanced:
- Reactants: 2 Mg, 2 O (from O₂)
- Products: 2 Mg, 2 O (from 2 MgO)
The balanced chemical equation is:
\[
\boxed{2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}}
\]
Answer
what is ___O2
Answered by
GPT-4o mini
In the chemical equation you provided, **O₂** represents molecular oxygen, which consists of two oxygen atoms bonded together. The underscores (___) before O₂ indicate that it is an unknown coefficient that needs to be determined in order to balance the equation properly.
In the context of balancing the equation:
- **O₂** is the reactant that provides oxygen for the reaction.
- The goal is to adjust the coefficient of O₂ so that the number of oxygen atoms on the reactants side matches the number on the products side.
When balancing the equation with magnesium (Mg) producing magnesium oxide (MgO), you ultimately find that the coefficient that balances O₂ is **1**, since you need one molecule of O₂ (which contains two oxygen atoms) to produce two molecules of MgO (each containing one oxygen atom).
Thus,
\[
\text{The balanced equation is: } 2 \text{Mg} + 1 \text{O}_2 \rightarrow 2 \text{MgO}
\]
In summary:
- **O₂** indicates diatomic oxygen.
- The coefficient before O₂ is typically determined when balancing the chemical equation. In this case, it was found to be **1**.
In the context of balancing the equation:
- **O₂** is the reactant that provides oxygen for the reaction.
- The goal is to adjust the coefficient of O₂ so that the number of oxygen atoms on the reactants side matches the number on the products side.
When balancing the equation with magnesium (Mg) producing magnesium oxide (MgO), you ultimately find that the coefficient that balances O₂ is **1**, since you need one molecule of O₂ (which contains two oxygen atoms) to produce two molecules of MgO (each containing one oxygen atom).
Thus,
\[
\text{The balanced equation is: } 2 \text{Mg} + 1 \text{O}_2 \rightarrow 2 \text{MgO}
\]
In summary:
- **O₂** indicates diatomic oxygen.
- The coefficient before O₂ is typically determined when balancing the chemical equation. In this case, it was found to be **1**.