Summary

If the amount of gas in a container is increased, the volume increases. If the amount of gas in a container is decreased, the volume decreases. If you heat a gas you give the molecules more energy so they move faster. This means more impacts on the walls of the container and an increase in the pressure.

There are several ways to increase the number of collisions.

1. You could add more molecules.
2. You could increase the temperature.
3. You could decrease the size of the container, this would force the molecules into a smaller area and therefore increase the number of collisions that take place.

1. An increase in the number of gas molecules in the same volume container increases pressure.
2. A decrease in container volume increases gas pressure.
3. An increase in temperature of a gas in a rigid container increases the pressure.

Molecules of a gas move randomly. In a sealed container they exert a force when they collide with the container walls and this applies a pressure to the container. If the cylinders heat up enough, their pressure will increase and they will explode. …

Heating a gas increases the kinetic energy of the particles, causing the gas to expand. In order to keep the pressure constant, the volume of the container must be increased when a gas is heated. This law explains why it is an important safety rule that you should never heat a closed container.

This shows that the pressure of a gas is inversely proportional to its volume. It means that for a gas at a constant temperature, pressure × volume is also constant. So increasing pressure from pressure 1 to pressure 2 means that volume 1 will change to volume 2, providing the temperature remains constant.

Gas. The atoms and molecules in gases are much more spread out than in solids or liquids. A gas will fill any container, but if the container is not sealed, the gas will escape. Gas can be compressed much more easily than a liquid or solid.

Gases have a negligible intermolecular force of attraction between the particles of gas. As a result, the random motion of particles in all directions is experiencing in the vessel. Hence, the gas fills the vessel in which it is kept.

As compression proceeds, the speed of the molecules and the distances between them continue to decrease, until eventually the substance undergoes change of state and becomes liquid. Although before the 19th cent.

During compression, the volume (V) of a gas decreases. When this happens, the pressure (P) of the gas increases if the number of moles (n) of gas remains constant. If you keep the pressure constant, reducing the temperature (T) also causes the gas to compress.

When an ideal gas is compressed in a closed container it raises the internal energy U. Compressing an ideal gas increases its temperature and its internal energy increases since U=f(t) for an ideal gas. Hence, when an ideal gas is compressed in a closed container its U increases.

According to Boyle’s law, “The volume of a gas is inversely proportional to pressure keeping the temperature the same”. Hence, when the gas is compressed, its molecules come closer and internal energy of gas is increased and the number of collisions will also increase.

If a gas is cooled, its particles will eventually stop moving about so fast and form a liquid. This is called condensation and occurs at the same temperature as boiling. Evaporation is dependent on individual particles gaining enough energy to escape the surface of the liquid and become gas particles.

This is called evaporation. If water vapour (gas) is cooled, it changes to water (liquid). This change is called condensing. Heat melts a solid and turns it into a liquid.

There is a loss of thermal energy. The gas particles also lose kinetic energy and they tend to move slower. The interparticle space that exists between the gas particles decreases. As it continues to cool down the gas will change to a liquid state.

But if we lower the temperature below 0 degrees Celsius, or 32 degrees Fahrenheit, water changes its phase into a solid called ice. Similarly, if we heat a volume of water above 100 degrees Celsius, or 212 degrees Fahrenheit, water changes its phase into a gas called water vapor.

As a liquid is heated, its vapor pressure increases until the vapor pressure equals the pressure of the gas above it. Bubbles of vaporized liquid (i.e., gas) form within the bulk liquid and then rise to the surface where they burst and release the gas.

Examples of Gas to Solid: 1. Making dry ice or solid carbon dioxide involves the removal of gaseous carbon dioxide from air and using cold temperatures and higher pressure causes the gas particles to skip the liquid phase and deposit into a solid to form a chunk of dry ice.

Gas (water vapor) If liquid water is boiled, it turns into a gas called water vapor.

Liquid helium boiling into gaseous helium. 4.) Mercury evaporating into… well, mercury fumes.

Phase Transition: Solid to Gas. Sublimation is the process of transformation directly from the solid phase to the gaseous phase, without passing through an intermediate liquid phase.

Deposition is the phase transition in which gas transforms into solid without passing through the liquid phase. Deposition is a thermodynamic process. The reverse of deposition is sublimation and hence sometimes deposition is called desublimation.

Sublimation: The process, where a solid on heating, directly changes into a gas without changing into liquid, and a gas on cooling, directly changes to solid without changing into liquid is called sublimation.

A mixture is a combination of two or more substances, where these substances are not bonded (or joined) to each other and no chemical reaction occurs between the substances….

Under certain circumstances, gas can transform directly into a solid. This process is called deposition. Water vapor to ice – Water vapor transforms directly into ice without becoming a liquid, a process that often occurs on windows during the winter months.

Those 11 gases are Helium, Argon, Neon, Krypton, Radon, Xenon, Nitrogen, Hydrogen, Chlorine, Fluorine, and Oxygen. These are called pure gases as they are all elements. You can use these names as the perfect example of gas matter.