Chem gasses quiz 1

1. Gasses are compressible. The volume of gasses decreases when pressure is exerted on the gas because molecules are more spread out in gasses than in liquids.

2. Gasses expand as temperature is increased and the the pressure remains constant. Because the molecules are moving and have more kinetic energy.

3. Gasses have a low viscosity. Which means a low resistance to flow. This means they can move through pipes more freely than liquids and can escape small openings in containers.

4. Gasses have much lower densities than solids and liquids. There is more space between molecules.

5. gases are miscible. They mix completely and evenly with each other when put in the same container.

Its used to provide a scientific model for explaining the behaviour of gasses.

ideal gas: a hypothetical gas that obeys the laws perfectly under any condition

real gas: differ from an ideal gas under certain conditions such as increased or lower temperature.

• 1. Ideal gasses- Gas molecules are very far apart compared to their small molecular size.
• real gasses- for high pressures, the molecules are forced closer together and their molecular size is bigger.

• 2. ideal gasses- gas molecules are in constant, random, straight-line motion because no force exists between them.
• real gasses- as the temperature decreases, the molecules slow down and the intermolecular attractions may cause molecules to stick together and the gases may become liquids.

• 3. ideal gasses- Gas molecules have perfectly elastic collisions in which no energy is lost and the collision occur quickly.
• real gasses- shapes of molecules change during collisions occurring more slowly. Meaning the pressure of the gas is less than ideal.

a measure of the force exerted by moving gas per unit of area

the force per unit of area exerted by air on all objects

Pa and 1 pa is equal to 1 N/m^2

Atm and 1 atm is equal to 101.325Kpa

mm hg and 760 mm hg is equal to 1 atm which is 101.325 Kpa

torr and 1 torr is equal to 1 mm Hg

Temp- measurement of the average kinetic energy of particles, the more kinetic energy the particles have the higher the temperature 

heat- total kinetic energy of a system

lowest possible temperature where the kinetic energy of all entities would be theoretically 0. Zero K is -237.15 degrees

celsius to kelvin- T= t + 273.15

kelvin to celsius- t= T - 273.15

Standard temperature and pressure is 273.15 K or zero degrees at 100Kpa 

Standard ambient temperature and pressure is 298.15 K or 25 degrees at 100 KPa

states when measured at the same temperature and pressure, the gaseous reactants and products of the chemical reaction are always in simple ratios of whole numbers. Avogadro's law helps prove this because equal volume of gases at the same temperature and volume will contain equal numbers of molecules.

States that as the pressure on a gas increases, the volume of the gas decreases. If the temperature and chemical amount of gas remains constant. This means volume is inversely proportional to pressure.

Decreasing the volume results inmate collisions between gas molecules and the container increasing pressure.

States that as the temperature increases the volume also increases this being proportional. If pressure and chemical amount of gas remains constant

States that the product of the pressure and volume of a gas is proportional to its temperature in kelvin when chemical amount remains constant.

R is 8.314 kpa*L/mol*K

Relationship between pressure volume temp and chemical amount of matter.