Gas Laws - Mixed Practice

What is STP?

• 1 Degrees Celsius and 0 ATM

• 0 Degrees Celsius and 1 ATM

• 0 Kevin and 10 ATM

• 273 Celsius and 273 ATM

Adding heat to a non-flexible container of gas will cause

• the molecules to slow and down hit the sides less often. The pressure will decrease.

• the container to explode.

• the molecules to speed up and hit the sides more often. The pressure will increase.

Tags

NGSS.HS-PS3-2

Adding more gas molecules to an equal size container held at a steady temperature will:

• Increase the pressure because there are more molecules, and therefore the sides of the container will be hit more often.

• not affect the pressure.

• Increase the pressure because the molecules will be moving faster.

What is happening as you move from volume 1 to volume 2?

• The pressure is held constant

• There are the same number of molecules in a smaller container, so volume 2 will have a higher pressure because the molecules are hitting the sides more often.

• There are more molecules in volume 2, which would cause them to be hotter and move faster, therefore pressure is increased.

• Volume 1 would have a higher pressure.

How do you convert mmhg to ATM?

• Multiply the mmhg pressure value by 760

• No need to convert--they can be used interchangeably.

• Divide the mmhg pressure value by 760.

How do you convert a kPA pressure value to ATM?

• No need to convert--use them interchangeably.

• Divide the kPA pressure value by 101.325

• Multpily the KPA pressure value by 101.325

Which formula would you use to answer the following problem?

At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?

• PV=nRT

• P1V1/T1=P2V2/T2

• Not enough information is given.

Which formula would you use to solve the following equation?

If I have 23 L of Ar at a pressure of 12 atm and a temperature of 200 K, and then I increase the pressure to 14 atm and the temperature to 300 K, what is my new volume?

• PV=nRT

• Not enough information is given.

• P1V1/T1 = P2V2/T2

If I have a flexible container of gas, which of the following is true?

• If I remove some of the gas molecules, the container will increase in size.

• The pressure on the inside of the container will be equal to the pressure outside the container.

• If I heat up the gas molecules, the container will decrease in size.

When using the ideal gas law (PV=nRT), how does the type of gas being examined affect the outcome?

• It has no affect--the formula is a good approximation for all gases.

• You need to pay close attention to the type of gas--Helium and the Noble gases use a different equation

• Because each gas has a unique molecular mass, that difference needs to be accounted for.

• Using an isotope or an ion will change your results.