States Of Matter

Question 1

Effect Of Temperature & Pressure On Gas

Answer 1

Temperature: Increasing the temperature of a gas increases the average kinetic energy of its particles. Higher kinetic energy means the particles move faster and collide with the container walls more frequently and with greater force. As a result, the volume of the gas increases because the particles push against the walls more forcefully, expanding the space they occupy.

Pressure: Increasing the pressure on a gas compresses its volume. When pressure increases, the gas particles are forced closer together, reducing the space between them. This happens because the particles collide more frequently with the container walls, exerting greater force over a smaller area. As a result, the gas volume decreases due to the reduced space available for particle movement.

Question 2

Diffusion

Answer 2

• Movement of particles from high to low concentration.
• Occurs due to constant random motion of particles.
• Particles spread out evenly over time.

Question 3

Effect of Relative Molecular Mass on Rate of Diffusion

Explain NH3 & HCL

Answer 3

• Gases with lower molecular mass diffuse more quickly.
• Lighter gas molecules have higher average speeds.
• They collide more frequently, facilitating faster diffusion.
• Heavier gas molecules move more slowly and diffuse more slowly.

EG: NH3 & HCL
The ammonia gas, having a lower molecular weight than the hydrogen chloride, will diffuse faster and travel a greater length of the tube.

Consequently, the white ring of ammonium chloride will form much closer to hydrochloric acid end of the tube.