Answer:
Explanation:
Okay, let's think through this step-by-step:
* Initial temperature (T1) = 567 K
* Final temperature (T2) = 269 K
* Initial volume (V1) = 22.4 L
* Final volume (V2) = 34.4 L
* We want to find the final pressure (P2)
We can use the combined gas law:
P1V1/T1 = P2V2/T2
* We don't know initial pressure P1, but we can cancel it out:
P1 * (V1/T1) = P2 * (V2/T2)
* Plug in the values:
P1 * (22.4 L / 567 K) = P2 * (34.4 L / 269 K)
* Solve for P2:
P2 = P1 * (22.4 L / 567 K) / (34.4 L / 269 K)
* The P1 terms cancel out, leaving:
P2 = (22.4 L / 567 K) / (34.4 L / 269 K)
P2 = 0.865
* Convert to atmospheres:
0.865 * 1 atm/1.013 bar = 0.854 atm
Therefore, the final pressure is 0.854 atmospheres.
