Gas Heating via Kinetic Theory

Steps:

• Sunlight warms the sealed cylinder, raising the gas temperature.
• Higher temperature increases the average kinetic energy of gas particles.
• Faster-moving particles collide with cylinder walls more frequently and with greater force.
• This raises internal pressure until the cylinder ruptures.

Why C is correct:

• Kinetic molecular theory states average kinetic energy is directly proportional to temperature (KE = 3/2 kT), so heating boosts speed, impact force, and collision rate.

Why the others are wrong:

• A: Gas particles are point masses with negligible, constant size; they don't expand.
• B: Particles don't grow larger; explosion stems from energy, not size change.
• D: Losing kinetic energy lowers temperature and pressure, preventing explosion.

Final answer: C