Final answer:
To determine the final temperature of a sulfur hexafluoride gas sample when the pressure changes, use Gay-Lussac's Law. With initial conditions of 50 Pa and 2500 K (possibly a typo), and a final pressure of 600 Pa, the new temperature is calculated as 30000 K, which seems unrealistic, indicating a potential error in the initial given temperature.
Step-by-step explanation:
The question relates to the calculation of the final temperature of a sample of sulfur hexafluoride gas (assumed typo for SF should be SF6) when the pressure is decreased, given the initial temperature and pressure. According to Gay-Lussac's Law, at constant volume, the pressure of a gas is directly proportional to its temperature in kelvins.
Given:
- Initial pressure P1 = 50 Pa
- Initial temperature T1 = 2500 K (assuming the typo meant 25.00, as 2500 seems unrealistic)
- Final pressure P2 = 600 Pa
We can use the formula
P1/T1 = P2/T2
to solve for the final temperature T2:
T2 = (P2 × T1) / P1
T2 = (600 Pa × 2500 K) / 50 Pa
T2 = 30000 K
This is an ideal gas law calculation that ignores the effects of gas non-idealities or phase changes. As the calculation stands, the result suggests a significant and unrealistic increase in temperature. If the initial temperature was intended to be 25.00 degrees Celsius or 298 K, the recalculation would yield T2 = (600 Pa × 298 K) / 50 Pa = 3576 K.