Test: Kinetic Particle Model of Matter - 2 - Year 11 MCQ

The Kinetic Theory of Matter posits that all matter is composed of minuscule particles in constant motion. This theory suggests that the particles making up matter are always moving, even if we can't see this movement with the naked eye. This concept helps explain various phenomena in chemistry and physics, highlighting the dynamic nature of even seemingly still substances.

Brownian motion describes the random and erratic movement of particles within a liquid or gas. This movement is induced by continuous collisions with smaller, often invisible particles. Observing Brownian motion provides insights into the dynamic and chaotic nature of particle interactions at a microscopic level, contributing to our understanding of the behavior of matter.

The Kelvin temperature scale commences at absolute zero, where 0 K represents the lowest possible temperature where atomic motion theoretically ceases. Absolute zero is a fundamental concept in thermodynamics, indicating the point at which particles have minimal energy and do not exhibit any thermal motion. This scale provides a precise measurement system for temperature, especially in scientific contexts.

Boyle's Law states that when the pressure on a gas increases, its volume decreases proportionally, provided the temperature remains constant. This inverse relationship between pressure and volume is crucial in understanding the behavior of gases under different conditions. As pressure rises, gas molecules get closer together, leading to a reduction in volume to maintain equilibrium.

The concept of Brownian motion primarily refers to the erratic movement of particles within a liquid or gas, induced by collisions with smaller particles. This phenomenon was first observed by Scottish scientist Robert Brown in the erratic movement of pollen grains in water under a microscope.

The Kelvin temperature scale starts at absolute zero, where 0 K corresponds to -273 degrees Celsius. Unlike the Celsius scale, the Kelvin scale does not have negative temperatures, making it particularly useful for scientific calculations involving temperature.

According to Boyle's Law, when the pressure on a gas increases, its volume decreases. This law describes the relationship between the pressure and volume of an ideal gas when the temperature remains constant.

When the temperature of a gas increases at constant volume, the pressure also increases. This is because higher temperatures lead to faster molecular movement, resulting in more frequent collisions with the container walls, thereby increasing the pressure.

A vacuum pump decreases the volume of a gas in a sealed container by extracting air, which in turn reduces the pressure inside the container, causing the gas to occupy less space.

The Gas Laws dictate that pressure increases when volume decreases and vice versa when the temperature remains constant. This principle is fundamental to understanding how gases behave under different conditions.