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WorksheetsCombined and Ideal Gas Laws
Total questions: 15
Worksheet time: 8mins
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.
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.
How do you handle base ten exponents in a multiplication problem?
Multiply the exponents
Subtract the exponents.
Add the exponents.
Ignore them entirely.
In a division problem involving base ten exponents, you should:
Subtract the exponents.
Divide the exponents.
Let your calculator figure it out.
Which of the following is true about this image?
The balloons are equal in air pressure to each other.
Hot air caused the molecules in the red balloon to speed up, expanding the volume.
The pressure on the inside of the balloon is equal to the pressure on the outside of the balloon.
All are true.
None are true.
When using a sealed, non-flexible container, the outside air pressure
has no affect on the inside pressure.
will always be greater than the inside pressure.
must be equal to the inside pressure.
If you have a balloon, and you increase both the temperature of the molecules and the outside pressure, what would happen?
The balloon would immediately explode.
The balloon may actually decrease in volume.
Increasing the temperature would always result in increased volume.
