Final answer:
Using Boyle's Law, which shows the inverse relationship between pressure and volume of a gas at a constant temperature, the volume of a gas will decrease to about 1.43 liters as the pressure increases from 1.00 atm to 3.50 atm.
Step-by-step explanation:
The student's question is related to the behavior of gases under different pressures at a constant temperature, which can be analyzed using Boyle's Law. Boyle's Law states that the volume of a fixed amount of gas kept at a constant temperature is inversely proportional to the pressure it exerts. When the pressure on a sample of gas increases, its volume decreases; conversely, as the pressure decreases, its volume increases. This relationship can be expressed by the equation P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, respectively, and P2 and V2 are the final pressure and volume, respectively.
In this case, the initial conditions are a volume (V1) of 5.00 liters and a pressure (P1) of 1.00 atm. The final pressure (P2) is given as 3.50 atm, and we want to find the new volume (V2). The equation can be rearranged to solve for V2:
V2 = (P1V1) / P2 = (1.00 atm × 5.00 L) / 3.50 atm = 5.00 L / 3.50 = approximately 1.43 liters.
Therefore, when the pressure on the gas increases from 1.00 atm to 3.50 atm at a constant temperature of 25.0 degrees C, the volume of the gas will decrease to approximately 1.43 liters.