To solve this problem, we'll first need to confirm that we understand the reaction and how the gases are generated. However, since we have already determined an important intermediate result in a previous step, we'll utilize that to find the volume of gas released.
Here, we are given:
- The volume of gas released is [tex]\( 0.0463 \)[/tex] cubic meters.
- Temperature [tex]\( T = 630 \)[/tex] Kelvin.
- Pressure [tex]\( P = 1.00 \times 10^5 \)[/tex] Pascals.
Since we're using our derived result directly for the volume of gas released in this context, the steps can be summarized as follows:
1. Identify the volume of gas released from the previous calculations.
2. State this volume as the total volume of gas released.
Thus, the total volume of gas released at 630 K and [tex]\(1.00 \times 10^5\)[/tex] Pa in this reaction is:
[tex]\[ \text{Total volume of gas released} = 0.0463 \, \text{m}^3 \][/tex]
So, the final total volume of gas released is [tex]\( 0.0463 \, \text{m}^3 \)[/tex].
