Think about the different rules that describe how gases behave. to do this, refer to what you have learned about the two principles concerning pressure and the three gas laws. summarize what each of these five rules state about the behavior of gases. then, give an example of a practical application for each one. (pressure)

Described down below.

Explanation:

Hello,

- Boyle's law: correlation between pressure and volume (assuming temperature and amount of gas remain constant). One common use of Boyle’s law is to predict the new volume of a gas when the pressure is changed (at constant temperature), or vice versa

- Charles' law: correlation between temperature and volume (assuming pressure and amount of gas remain constant). It is used to prove that the absolute 0 unattainable (T=0K).

- Avogadro's law: correlation between amount of gas and volume (assuming temperature  and pressure p remain constant). As an example, since we can blow up a basketball, we are adding more gas molecules into it. The more gaseous molecules, the greater the volume.

- Dalton's law: correlation that states that for a mixture of gases in a container, the total pressure exerted is the addition among each pressure that each gas would exert if it were alone. It is useful to analyze the effects of which partial pressure might have on scuba divers. While the total gas pressure increases as a diver increases their descent, the partial pressure of each gas involved increases as well which might cause harm to the diver’s body if proper actions are not carried out.

- Gay-Lussac's law: it states that when the temperature of a sample of gas in a rigid container is increased, the pressure of the gas increases as well. An interesting example is shown when gun pin strikes, because it ignites the gun powder and this increases the temperature which in turn increases the pressure and bullet is fired from the gun.

Best regards.

the correct option is c.

isotopes refers to different forms of the same element with the same atomic number but different mass number as a result of difference in their neutron numbers. isotopes have different relative atomic mass but share the same chemical properties.