Physics · Fluid Dynamics
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Pressure of a gas is directly proportional to:
- A
Average K.E. of its molecules
- B
Average vibrational K.E. of its molecules
- C
Average translational K.E. of its molecules
- D
All of the above
The pressure of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules.
This is based on the kinetic molecular theory of gases, which states that:
1. Gas molecules are in constant random motion.
2. The molecules collide with each other and the container walls.
3. The collisions with the walls cause the pressure exerted by the gas.
The average translational kinetic energy of the molecules is directly related to the temperature of the gas. As the temperature increases, the molecules move faster and have more kinetic energy.
The pressure (P) of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules, which can be expressed mathematically as:
P ∝ K.E.
or
P = (2/3) × (K.E.) × (density of the gas)
This means that if the average translational kinetic energy of the molecules increases, the pressure of the gas also increases.
This relationship is a fundamental principle in the behavior of gases and is a key concept in understanding the properties of gases.
The pressure of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules.
This is based on the kinetic molecular theory of gases, which states that:
1. Gas molecules are in constant random motion.
2. The molecules collide with each other and the container walls.
3. The collisions with the walls cause the pressure exerted by the gas.
The average translational kinetic energy of the molecules is directly related to the temperature of the gas. As the temperature increases, the molecules move faster and have more kinetic energy.
The pressure (P) of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules, which can be expressed mathematically as:
P ∝ K.E.
or
P = (2/3) × (K.E.) × (density of the gas)
This means that if the average translational kinetic energy of the molecules increases, the pressure of the gas also increases.
This relationship is a fundamental principle in the behavior of gases and is a key concept in understanding the properties of gases.
The pressure of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules.
This is based on the kinetic molecular theory of gases, which states that:
1. Gas molecules are in constant random motion.
2. The molecules collide with each other and the container walls.
3. The collisions with the walls cause the pressure exerted by the gas.
The average translational kinetic energy of the molecules is directly related to the temperature of the gas. As the temperature increases, the molecules move faster and have more kinetic energy.
The pressure (P) of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules, which can be expressed mathematically as:
P ∝ K.E.
or
P = (2/3) × (K.E.) × (density of the gas)
This means that if the average translational kinetic energy of the molecules increases, the pressure of the gas also increases.
This relationship is a fundamental principle in the behavior of gases and is a key concept in understanding the properties of gases.
The pressure of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules.
This is based on the kinetic molecular theory of gases, which states that:
1. Gas molecules are in constant random motion.
2. The molecules collide with each other and the container walls.
3. The collisions with the walls cause the pressure exerted by the gas.
The average translational kinetic energy of the molecules is directly related to the temperature of the gas. As the temperature increases, the molecules move faster and have more kinetic energy.
The pressure (P) of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules, which can be expressed mathematically as:
P ∝ K.E.
or
P = (2/3) × (K.E.) × (density of the gas)
This means that if the average translational kinetic energy of the molecules increases, the pressure of the gas also increases.
This relationship is a fundamental principle in the behavior of gases and is a key concept in understanding the properties of gases.
The pressure of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules.
This is based on the kinetic molecular theory of gases, which states that:
1. Gas molecules are in constant random motion.
2. The molecules collide with each other and the container walls.
3. The collisions with the walls cause the pressure exerted by the gas.
The average translational kinetic energy of the molecules is directly related to the temperature of the gas. As the temperature increases, the molecules move faster and have more kinetic energy.
The pressure (P) of a gas is directly proportional to the average translational kinetic energy (K.E.) of its molecules, which can be expressed mathematically as:
P ∝ K.E.
or
P = (2/3) × (K.E.) × (density of the gas)
This means that if the average translational kinetic energy of the molecules increases, the pressure of the gas also increases.
This relationship is a fundamental principle in the behavior of gases and is a key concept in understanding the properties of gases.
Tagged under Physics · Fluid Dynamics · 2017