Answer :
To find the final chemical equation from the given intermediate reactions, we need to manipulate the intermediate reactions to see how they combine to produce a balanced final equation. Here are the intermediate reactions provided:
1. [tex]\( P_4O_6(s) \rightarrow P_4(s) + 3O_2(g) \)[/tex]
2. [tex]\( P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \)[/tex]
Let's sum these two intermediate equations step-by-step and simplify where possible:
1. Write down the equations:
[tex]\[ \begin{array}{l} P_4O_6(s) \rightarrow P_4(s) + 3O_2(g) \\ P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \end{array} \][/tex]
2. Combine the two equations:
When combining chemical equations, the intermediate species produced in one step and consumed in the following step can be canceled out. Here, [tex]\(P_4(s)\)[/tex] appears as a product in the first equation and as a reactant in the second equation, so [tex]\(P_4(s)\)[/tex] can be canceled out.
After adding both equations, we get:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4(s) + 3O_2(g) + P_4O_{10}(s) \][/tex]
3. Simplify by canceling common species:
Now, cancel out the common intermediate species on both sides of the equation. Here [tex]\(P_4(s)\)[/tex] appears on both the left-hand side and right-hand side, so they cancel out. Similarly, we can simplify the oxygen molecules:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) + 3O_2(g) \][/tex]
Finally, rearranging and combining the oxygen molecules, we get:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
Thus, the balanced final chemical equation is:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
This final equation is not among the given options in your list, which means that none of the provided options are correct. However, based on the intermediate steps, we confirm that the balanced final equation is indeed:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
1. [tex]\( P_4O_6(s) \rightarrow P_4(s) + 3O_2(g) \)[/tex]
2. [tex]\( P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \)[/tex]
Let's sum these two intermediate equations step-by-step and simplify where possible:
1. Write down the equations:
[tex]\[ \begin{array}{l} P_4O_6(s) \rightarrow P_4(s) + 3O_2(g) \\ P_4(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \end{array} \][/tex]
2. Combine the two equations:
When combining chemical equations, the intermediate species produced in one step and consumed in the following step can be canceled out. Here, [tex]\(P_4(s)\)[/tex] appears as a product in the first equation and as a reactant in the second equation, so [tex]\(P_4(s)\)[/tex] can be canceled out.
After adding both equations, we get:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4(s) + 3O_2(g) + P_4O_{10}(s) \][/tex]
3. Simplify by canceling common species:
Now, cancel out the common intermediate species on both sides of the equation. Here [tex]\(P_4(s)\)[/tex] appears on both the left-hand side and right-hand side, so they cancel out. Similarly, we can simplify the oxygen molecules:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) + 3O_2(g) \][/tex]
Finally, rearranging and combining the oxygen molecules, we get:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
Thus, the balanced final chemical equation is:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
This final equation is not among the given options in your list, which means that none of the provided options are correct. However, based on the intermediate steps, we confirm that the balanced final equation is indeed:
[tex]\[ P_4O_6(s) + 5O_2(g) \rightarrow P_4O_{10}(s) \][/tex]
