To solve for the final chemical equation from the given intermediate chemical equations, we will follow each step carefully to combine and simplify the equations.
We are given the following intermediate chemical equations:
1. [tex]\( P_4O_{10}(s) \rightarrow P_4(s) + 3O_2(g) \)[/tex]
2. [tex]\( P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \)[/tex]
Our goal is to combine these equations to form a single balanced equation. Let's go through the steps:
### Step 1: Write down each equation.
[tex]\[
\text{Equation 1: } P_4O_{10}(s) \rightarrow P_4(s) + 3O_2(g)
\][/tex]
[tex]\[
\text{Equation 2: } P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s)
\][/tex]
### Step 2: Add the two equations together.
When adding chemical equations together, we simply add the reactants and the products.
[tex]\[
P_4O_{10}(s) \rightarrow P_4(s) + 3O_2(g)
\][/tex]
[tex]\[
+ \, P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s)
\][/tex]
Combining the equations:
[tex]\[
P_4O_{10}(s) + P_4(s) + 3O_2(g) + 5O_2(g) \rightarrow P_4(s) + P_4O_{10}(s)
\][/tex]
### Step 3: Combine like terms to simplify the equation.
[tex]\[
P_4O_{10}(s) + P_4(s) + 3O_2(g) + 5O_2(g) \rightarrow P_4(s) + P_4O_{10}(s)
\][/tex]
Combine the oxygen terms:
[tex]\[
P_4O_{10}(s) + P_4(s) + 8O_2(g) \rightarrow P_4(s) + P_4O_{10}(s)
\][/tex]
### Step 4: Cancel out the same substances on both sides.
We can cancel out [tex]\( P_4O_{10}(s) \)[/tex] and [tex]\( P_4(s) \)[/tex] from both sides of the equation:
[tex]\[
P_4O_{10}(s) + 8O_2(g) \rightarrow P_4O_{10}(s) + P_4(s)
\][/tex]
### Result:
The final balanced chemical equation is:
[tex]\[
P_4O_{10}(s) + 8O_2(g) \rightarrow P_4O_{10}(s) + P_4(s)
\][/tex]
This equation shows the reactants and products in a balanced form, detailing the transformation processes in the given chemical reactions.
