Suppose a sample of gas is in a flexible container. If the temperature is held constant, and you add some gas molecules to the container, would the volume of the container need to increase, decrease, or remain unchanged in order to keep the pressure constant? Explain your answer in your own words using only kinetic-molecular theory. Do not use any equations or gas laws or math. Be detailed and complete in your explanation.

A sample of nitrogen gas at 310 K and 1.01 atm occupies a volume of 1.51 L. If the gas is compressed into a smaller volume, while at the same time it is cooled to a lower temperature, the final gas pressure ? will be lower than 1.01 atm. ? will be higher than 1.01 atm. ? could be higher or lower than 1.01 atm depending on the final volume and temperature.

A sample of gas takes up 3.5 liters, at a pressure of 0.75 atmospheres and a temperature of 525 degrees Kelvin.  If the sample is cooled to 250 degrees and the pressure drops to 0.25 atmospheres, what is the new volume of the gas?

A sample of gas contains has a pressure of 1.40 atm at 40.0 mL. What is the pressure of the sample in atmospheres if the volume decreases to 11 mL under constant moles and temperature? Do not include units when entering your answer.

In the gas laws experiment we observed how canging certain varibles had an effect on a sample of contained gas. Display your understanding of the gas laws by designing a example of an experiment in which displays the effect of pressure on a gas.

A 3.66 L bicycle tire has a pressure of 5.71 atm.  All of the air in the bicycle tire is transferred to a car tire which has a volume of 10.0 L.  Calculate the pressure, in atm, inside the car tire.

A gas occupies a volume of 1.25 L at a pressure of 5.50 atm, what will be the pressure (atm) of the gas if the volume is expanded to 4.69 L while the gas sample is held at constant temperature?