Chemistry - Investigation 4, Experience 1

Kinetic energy

The energy an object has due to its motion.

Properties of matter

Kinetic energy of the particles that make up the substance.

Kinetic theory

All matter in tiny particles that are in constant motion.

Ideal gas

Small, hard spheres with insignificant volume. They are in motion (rapid, constant, and random) and colliding at room temperature. The collisions are elastic / have no loss of kinetic energy in collision. Particles move in strait lines until they collide with other particles or walls.

Standard temperature and pressure (STP)

A standard set oof conditions used for comparing properties of different gases and corresponds to a temperature of 0c and approximately atmospheric pressure at sea level.

Elements of common gases

All of the last group (He-Og), (F-Br), O, N, H, and Hg

Steam

Molecules of H2O breaking free from the bonds (hydrogen bonds) at 100C or higher, turning it into water vapor (gas).

Bromine

Particles in bromine are diatomic (2 bromine atoms), at temperatures 59.8C or above, Br2 is a gas.

Gas pressure

The result of forces (result of collision) between the molecules of gas and container walls. 

How can gas pressure increase?

Increase the number of collision by shrinking the container, changing the temperature, or adding more particles.

High temperature is gas pressure

Particles move faster and increases the probability of collision, so pressure is higher.

Low temperature in gas pressure

Particles of gas move slowly. They are less likely to collide, so pressure is lower.

Smaller space

Particles get closer and collision is likely, causing higher pressure.

More particles

Collison increases, causing higher pressure.