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Questions and Answers
What happens to the speeds of gas particles as they collide?
What happens to the speeds of gas particles as they collide?
- Their speeds change. (correct)
- They always speed up.
- They always slow down.
- Their speeds remain constant.
How is the average kinetic energy of gas molecules related to temperature?
How is the average kinetic energy of gas molecules related to temperature?
- Not related at all.
- Inversely proportional to absolute temperature.
- Directly proportional to absolute temperature. (correct)
- Directly proportional to pressure.
Under what conditions do real gases behave more like ideal gases?
Under what conditions do real gases behave more like ideal gases?
- Low temperature and high pressure.
- High temperature and low pressure. (correct)
- Low temperature and low pressure.
- High temperature and high pressure.
What effect does high pressure have on gas molecules?
What effect does high pressure have on gas molecules?
What does the volume occupied by the molecules affect?
What does the volume occupied by the molecules affect?
Which gas shows a decrease followed by an increase in pV with pressure?
Which gas shows a decrease followed by an increase in pV with pressure?
What is the first part of the equation relating preal and pideal?
What is the first part of the equation relating preal and pideal?
Why do real gases deviate from ideal gas behavior?
Why do real gases deviate from ideal gas behavior?
What is the mole fraction of CO2 in a mixture containing 54.0 grams of CO2 and 33.0 grams of N2?
What is the mole fraction of CO2 in a mixture containing 54.0 grams of CO2 and 33.0 grams of N2?
According to Graham's Law, what is the relationship between the effusion rate of a gas and its molecular mass?
According to Graham's Law, what is the relationship between the effusion rate of a gas and its molecular mass?
What does the kinetic molecular theory of gases state about the particles of a gas?
What does the kinetic molecular theory of gases state about the particles of a gas?
What is the partial pressure of CO2 in a gas mixture if its mole fraction is 0.51 and the total pressure is 101.3 kPa?
What is the partial pressure of CO2 in a gas mixture if its mole fraction is 0.51 and the total pressure is 101.3 kPa?
What does the assumption of negligible volume of gas molecules in kinetic molecular theory explain?
What does the assumption of negligible volume of gas molecules in kinetic molecular theory explain?
What occurs during collisions of gas molecules according to kinetic molecular theory?
What occurs during collisions of gas molecules according to kinetic molecular theory?
What is the total number of moles in a mixture containing 1.23 moles of CO2 and 1.18 moles of N2?
What is the total number of moles in a mixture containing 1.23 moles of CO2 and 1.18 moles of N2?
Which of the following statements correctly describes the movement of gas particles?
Which of the following statements correctly describes the movement of gas particles?
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Study Notes
Ideal Gas Behaviour
- The average kinetic energy of the particles of a gas is directly proportional to the absolute temperature
- Real gases act like ideal gases under high temperature and low pressure.
- At low pressures, real gases deviate from ideal gas behavior
- At high pressures, real gases deviate from ideal gas behavior
- The collisions of gas molecules are perfectly elastic
Deviation from Ideal Gas Behaviour
- Real gases deviate from the ideal gas law because the molecules are in constant random motion, have no force of attraction between each other at ordinary temperature and pressure and, the volume of the molecules is negligible in comparison with the empty space between them.
Dalton’s Law of Partial Pressures
- Total pressure of a mixture of gases is the sum of partial pressures of the individual gases
- The partial pressure of the gas is the pressure that the gas would exert if it alone occupied the whole volume
- The partial pressure of a gas is directly proportional to its mole fraction
Graham’s Law of Effusion
- The effusion rate of a gas is inversely proportional to the square root of its molecular mass.
- The rate of effusion is the rate a gas escapes through a small hole into a vacuum.
- The higher the molecular mass, the slower the rate of effusion
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