Find the best answers to your questions at Westonci.ca, where experts and enthusiasts provide accurate, reliable information. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform. Discover detailed answers to your questions from a wide network of experts on our comprehensive Q&A platform.
Sagot :
To balance the chemical equation [tex]\( \text{Mg} + \text{O}_2 \rightarrow \text{MgO} \)[/tex], we need to ensure that the number of atoms of each element is the same on both sides of the equation. Here's the step-by-step process to achieve this:
1. Identify the Reactants and Products:
- Reactants: Magnesium (Mg) and Oxygen (O[tex]\(_2\)[/tex])
- Products: Magnesium Oxide (MgO)
2. Write the Unbalanced Equation:
[tex]\[ \text{Mg} + \text{O}_2 \rightarrow \text{MgO} \][/tex]
3. Count the Atoms of Each Element on Both Sides:
- Left side:
- Mg: 1
- O: 2 (since [tex]\( O_2 \)[/tex] has 2 atoms of Oxygen)
- Right side:
- Mg: 1
- O: 1 (in MgO there is 1 atom of Magnesium and 1 of Oxygen)
4. Balance the Oxygen Atoms:
- On the left, we have 2 Oxygen atoms, while on the right, we have only 1. To balance the Oxygen atoms, we will need 2 Magnesium Oxide (MgO) molecules which will provide 2 Oxygen atoms:
[tex]\[ \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
- Now the equation looks like this:
- Left side: [tex]\(\text{Mg}: 1\)[/tex], [tex]\(\text{O}: 2\)[/tex]
- Right side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex]
5. Balance the Magnesium Atoms:
- On the left, we had only 1 Magnesium atom initially, but on the right, we now have 2 Magnesium atoms in 2 MgO. To balance the Magnesium atoms, we place a coefficient of 2 in front of Mg on the left:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
6. Final Balanced Equation:
- Double-check the counts of each type of atom to ensure they are the same on both sides:
- Left side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex],
- Right side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex]
Thus, the balanced equation is:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
Finally, among the given options:
- [tex]\( \text{Mg} + 2 \text{O}_2 \rightarrow 4 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + 2 \text{O}_2 \rightarrow 2 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + 2 \text{O}_2 \rightarrow 4 \text{MgO} \)[/tex]
The correct balanced equation is:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
The correct answer is:
[tex]\[ \boxed{2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}} \][/tex]
1. Identify the Reactants and Products:
- Reactants: Magnesium (Mg) and Oxygen (O[tex]\(_2\)[/tex])
- Products: Magnesium Oxide (MgO)
2. Write the Unbalanced Equation:
[tex]\[ \text{Mg} + \text{O}_2 \rightarrow \text{MgO} \][/tex]
3. Count the Atoms of Each Element on Both Sides:
- Left side:
- Mg: 1
- O: 2 (since [tex]\( O_2 \)[/tex] has 2 atoms of Oxygen)
- Right side:
- Mg: 1
- O: 1 (in MgO there is 1 atom of Magnesium and 1 of Oxygen)
4. Balance the Oxygen Atoms:
- On the left, we have 2 Oxygen atoms, while on the right, we have only 1. To balance the Oxygen atoms, we will need 2 Magnesium Oxide (MgO) molecules which will provide 2 Oxygen atoms:
[tex]\[ \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
- Now the equation looks like this:
- Left side: [tex]\(\text{Mg}: 1\)[/tex], [tex]\(\text{O}: 2\)[/tex]
- Right side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex]
5. Balance the Magnesium Atoms:
- On the left, we had only 1 Magnesium atom initially, but on the right, we now have 2 Magnesium atoms in 2 MgO. To balance the Magnesium atoms, we place a coefficient of 2 in front of Mg on the left:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
6. Final Balanced Equation:
- Double-check the counts of each type of atom to ensure they are the same on both sides:
- Left side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex],
- Right side: [tex]\(\text{Mg}: 2\)[/tex], [tex]\(\text{O}: 2\)[/tex]
Thus, the balanced equation is:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
Finally, among the given options:
- [tex]\( \text{Mg} + 2 \text{O}_2 \rightarrow 4 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + 2 \text{O}_2 \rightarrow 2 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \)[/tex]
- [tex]\( 2 \text{Mg} + 2 \text{O}_2 \rightarrow 4 \text{MgO} \)[/tex]
The correct balanced equation is:
[tex]\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \][/tex]
The correct answer is:
[tex]\[ \boxed{2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO}} \][/tex]
Thank you for your visit. We are dedicated to helping you find the information you need, whenever you need it. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.
