40 Questions
What is the characteristic of particles in an ideal gas?
They have a mass but occupy no volume
What is the unit of measurement for the number of particles in a gas?
Moles
What is the temperature scale used by scientists for calculations?
Kelvins
What is the force exerted by gas particles on the container walls?
Pressure
What is the accepted SI unit for gas pressure?
Pascal
What is the definition of pressure?
Force divided by area
What happens to the volume available to the gas when more gas particles are added to the cylinder?
The volume increases
Why does the piston rise when more gas particles are added to the cylinder?
Due to the greater force from collisions against the walls of the container
What is the relationship between the number of gas particles and volume according to Avogadro's Law?
The volume and the number of gas particles are directly proportional
What happens to the internal pressure when the piston rises?
It decreases
What happens to the pressure of a gas when its volume is decreased, while keeping the temperature and number of gas particles constant?
It increases
Why does the volume of your lungs increase when you breathe in?
Due to the expansion of the chest
What is the relationship between the pressure and volume of an ideal gas, if the temperature and number of gas particles are constant?
Inversely proportional
What is the purpose of the valve on the left of the apparatus?
To add or remove gas particles from the cylinder
What happens to the pressure of a gas when its volume is doubled, while keeping the temperature and number of gas particles constant?
It decreases to one-half its original value
What is the statement that describes the inverse relationship between the pressure and volume of an ideal gas?
Boyle's Law
What happens to the volume of a gas when its pressure is increased, while keeping the temperature and number of gas particles constant?
It decreases
Do real gases follow the exact mathematical relationship between pressure and volume described by Boyle's Law?
No, they deviate somewhat
Which equation is commonly memorized and written?
PV = nRT
What is the purpose of rearranging the ideal gas equation to isolate R?
To show the relationship between PV and nT
What does the ratio PV/nT always remain the same for?
For ideal gases, regardless of changes in their properties
What is the purpose of the expanded form of the ideal gas equation?
To find the mass of the gas in grams
What are the units of the standard gas containers used to fill luminous tubes?
Liters (L)
At what temperature and pressure are the standard gas containers filled?
22 °C and 101 kPa
What is the initial pressure of the gas in the standard container?
101 kPa
What is the final volume of the gas when it exerts a pressure of 1.3 kPa at 19 °C?
Cannot be determined with the given information
Which law can be used to find the final volume of the balloon when the pressure is reduced from 3 atmospheres to 0.5 atmospheres?
Boyle's law
What is the final volume of the balloon when the pressure is reduced from 3 atmospheres to 0.5 atmospheres?
12 L
What is the volume of the gas when it is compressed from 2.00 L to 1.00 L?
1.00 L
What is the purpose of converting the temperature from Celsius to Kelvin in the problem?
To use the ideal gas laws
The ideal gas equation is often written in the form PV = nRT.
True
The ratio of PV/nT always changes when the properties of an ideal gas change.
False
The expanded form of the ideal gas equation uses moles (n) instead of mass in grams (g) divided by molar mass (M).
False
The standard gas containers used to fill luminous tubes have a volume of 2.0 L.
False
Neon gas in luminous tubes radiates blue light.
False
R is a constant that varies depending on the pressure unit used.
False
The ideal gas equation is derived from the equation of state for real gases.
False
The ideal gas equation can be used to calculate changes in the properties of a real gas.
False
The temperature of the neon gas in the standard containers is 20 °C.
False
The pressure of the neon gas in the standard containers is 100 kPa.
False
Test your understanding of ideal gases and their properties in medical physics. Learn about the assumptions of ideal gases, including point masses and lack of intermolecular forces, and how they relate to volume, number of particles, temperature, and pressure.
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