Podcast
Questions and Answers
The average distance covered by a molecule between two successive collisions is called the ______.
The average distance covered by a molecule between two successive collisions is called the ______.
mean free path
Two phenomena that provide evidence of molecular motion are diffusion and ______.
Two phenomena that provide evidence of molecular motion are diffusion and ______.
Brownian motion
Avogadro's hypothesis states that the number of molecules in 22.4 litres of any gas is ______.
Avogadro's hypothesis states that the number of molecules in 22.4 litres of any gas is ______.
6.02 x 10^23
A real gas behaves like an ideal gas at low ______ and high temperature.
A real gas behaves like an ideal gas at low ______ and high temperature.
Boyle's law states that pressure (P) is inversely proportional to volume (V) at constant ______.
Boyle's law states that pressure (P) is inversely proportional to volume (V) at constant ______.
Charles law states that at constant pressure (P), volume (V) is directly proportional to temperature (T) on the ______ scale.
Charles law states that at constant pressure (P), volume (V) is directly proportional to temperature (T) on the ______ scale.
Dalton's law of partial pressures states that the total pressure of a mixture of gases is the sum of their ______ pressures.
Dalton's law of partial pressures states that the total pressure of a mixture of gases is the sum of their ______ pressures.
In kinetic theory, the universal gas constant R is the same for ______ gases.
In kinetic theory, the universal gas constant R is the same for ______ gases.
The formula for mean free path is T = ______, where d is the diameter of the molecule.
The formula for mean free path is T = ______, where d is the diameter of the molecule.
According to the equation n = PV/RT, 'n' represents the number of ______.
According to the equation n = PV/RT, 'n' represents the number of ______.
Flashcards
What is the mean free path?
What is the mean free path?
The average distance a molecule travels between two successive collisions.
Name two phenomena that prove molecular motion.
Name two phenomena that prove molecular motion.
Diffusion and Brownian motion provide conclusive evidence of molecular motion.
How does kinetic theory support Avogadro's hypothesis?
How does kinetic theory support Avogadro's hypothesis?
Avogadro's hypothesis states that equal volumes of ideal gases at the same temperature and pressure contain the same number of molecules. It follows that the Avogadro number, the number of molecules in 22.4 liters of any gas, is a constant value.
When does a real gas act ideally?
When does a real gas act ideally?
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State Boyle's law.
State Boyle's law.
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State Charles's law.
State Charles's law.
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What is Dalton's law of partial pressures?
What is Dalton's law of partial pressures?
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What is the formula for mean free path?
What is the formula for mean free path?
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Explain how diffusion and Brownian motion demonstrate molecular motion.
Explain how diffusion and Brownian motion demonstrate molecular motion.
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Study Notes
Mean Free Path
- The mean free path is the average distance a molecule travels between collisions.
- Formula: T = 1 / √(2πnd2)
- Where n is the number density and d is the molecule's diameter
Molecular Motion Evidence
- Two key phenomena demonstrating molecular motion are:
- Diffusion
- Brownian motion
Avogadro's Hypothesis
- Kinetic theory supports Avogadro's hypothesis by showing that the number of molecules per unit volume (or the number of moles) is the same for all gases at the same conditions of pressure, volume and temperature.
- This is because the universal gas constant (R) is the same for all gases, and from the ideal gas law: n = PV/RT.
Real Gas vs. Ideal Gas Behavior
- Real gases behave like ideal gases at low pressures and high temperatures.
- This is because when pressure is low, molecules are further apart and thus interactions between them are minimized. Similarly, when temperature is high the molecules move faster, making their interactions less significant.
Boyle's Law
- At constant temperature, the pressure of a gas is inversely proportional to its volume.
- Formula: P ∝ 1/V (or) PV = Constant
Charles's Law
- At constant pressure, the volume of a gas is directly proportional to its Kelvin temperature.
- Formula: V ∝ T (or) V/T = Constant
Dalton's Law of Partial Pressures
- The total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the individual gases.
- Formula: P = P1 + P2 + P3 + ...
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