Final answer:
The pressure of a gas at a new temperature of 273K, when initially it has a pressure of 3.5 atm at 200K, can be calculated using Gay-Lussac's Law. The new pressure is found to be approximately 4.78 atm when the volume remains constant.
Step-by-step explanation:
The question involves calculating the change in pressure of a gas when its temperature is increased while keeping its volume constant, based on the principles of ideal gas law. According to Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume is held constant, the new pressure can be calculated using the formula:
P1/T1 = P2/T2
Where:
- P1 is the initial pressure (3.5 atm)
- T1 is the initial temperature (200K)
- P2 is the final pressure
- T2 is the final temperature (273K)
By rearranging the equation and solving for P2, we can determine the new pressure:
P2 = P1 · (T2/T1)
P2 = 3.5 atm · (273K / 200K) = 3.5 atm · 1.365 = 4.7775 atm
The new pressure at 273K with constant volume is then approximately 4.78 atm.