Final answer:
If the pressure of a gas sample is increased from 3.25 atm to 12.5 atm while the volume remains constant, according to Gay-Lussac's law, the temperature will increase because the kinetic energy of the gas particles also increases.
Step-by-step explanation:
The question involves understanding the relationship between pressure and temperature for a gas, which can be described by Gay-Lussac's law and Charles's law. These gas laws are a part of thermodynamics and the study of ideal gases, which are typically covered in high school chemistry courses. In particular, Gay-Lussac's law states that for a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature.
If a sample of gas originally occupies 3.25 atm at 625 K and the pressure is increased to 12.5 atm, and assuming the volume is constant and we're dealing with an ideal gas, the temperature would also increase. Therefore, the correct answer is: A. It increases. The increase in temperature is due to the gas particles gaining kinetic energy as the pressure is increased, which according to the kinetic theory of gases, results in an increase in temperature.