What is the coefficient for aluminum after the following equation is balanced: Al(s) + O2(g) --> Al2O3(s)
options:
2
4
1
3
0
What is your problem in balancing this equation? It looks simple enough to me. It's a simple trial and error (ALTHOUGH it can be done by redox methods).
To balance the equation, you need to make sure that the number of atoms of each element is the same on both sides of the equation.
In the unbalanced equation:
Al(s) + O2(g) --> Al2O3(s)
There is one atom of aluminum on the left side and two atoms of aluminum on the right side. To balance the aluminum atoms, you need to place a coefficient of 2 in front of Al on the left side:
2 Al(s) + O2(g) --> Al2O3(s)
So, the coefficient for aluminum is 2. Hence, the correct option is:
2
To determine the coefficient for aluminum (Al) in the balanced equation Al(s) + O2(g) -> Al2O3(s), we need to balance the equation by ensuring that the same number of atoms of each element appear on both sides of the arrow.
1. Start by counting the number of atoms for each element on both sides of the equation. On the left side, we have 1 Al atom and 2 O atoms. On the right side, we have 2 Al atoms and 3 O atoms.
2. Since there is only 1 Al atom on the left side, we need to balance it by placing a coefficient in front of Al on the left side. Let's use "2" as the coefficient for Al: 2Al(s) + O2(g) -> Al2O3(s).
3. Now, let's recalculate the number of atoms for each element. On the left side, we have 2 Al atoms and 2 O atoms. On the right side, we have 2 Al atoms and 3 O atoms.
4. There are still more O atoms on the right side than the left side. To balance the O atoms, we need to place a coefficient in front of the O2 on the left side. Let's use "3" as the coefficient for O2: 2Al(s) + 3O2(g) -> Al2O3(s).
5. Recalculating the number of atoms, we have 2 Al atoms and 6 O atoms on both sides of the equation.
Therefore, the coefficient for aluminum (Al) in the balanced equation Al(s) + O2(g) -> Al2O3(s) is "2."