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Why does a gas exert pressure on the walls of its container?
Because gas molecules attract each other
Because gas molecules collide with the walls
Because the gas has high density
Because gas molecules expand on heating
Because gas molecules collide with the walls
Gas molecules exert pressure on the walls of a container because they are in constant, random motion and frequently collide with the inner surface of the container. These collisions impart force over the area of the wall, creating what we perceive as gas pressure.
Gas molecules exert pressure on the walls of a container because they are in constant, random motion and frequently collide with the inner surface of the container. These collisions impart force over the area of the wall, creating what we perceive as gas pressure.
Think of a room full of energetic toddlers constantly bouncing off the walls; the constant 'hits' they deliver to the wall surfaces are analogous to the pressure gas molecules exert on a container.
MPC: Motion, Particles, Collisions (Pressure)
P=AFтАЛ тАФ Pressure as force per unit area
F=dtdpтАЛ тАФ Newton's second law relating force to change in momentum
According to the Kinetic Molecular Theory of gases, gas particles possess kinetic energy and move in straight lines until they strike a boundary. Upon collision, the particles undergo a change in momentum (dp) over a time interval (dt). According to Newton's Second Law, the force exerted is defined as F=dtdpтАЛ, and since Pressure (P) is Force per unit area (A), it is expressed as P=AFтАЛ.
Gas pressure is directly proportional to the frequency and force of collisions.
Temperature increase raises the average kinetic energy of molecules, leading to more forceful and frequent collisions.
Pressure is a macro-scale result of billions of micro-scale molecular impacts.
Inflation of automobile tires
Functionality of pressure cookers
Standard atmospheric pressure at sea level is 1.013├Ч105┬аPa.
Option A is incorrect because attractive forces (Van der Waals forces) are generally weak in ideal gases and reduce rather than cause pressure. Option C is incorrect as density influences pressure only through collision frequency, not as the root cause. Option D is incorrect because thermal expansion is a consequence of increased kinetic energy and pressure, not the cause of wall pressure.
B is correct тАФ Gas molecules exert pressure due to the continuous bombardment and momentum transfer occurring during collisions with the container walls.
Always remember that in ideal gas problems, assume collisions with walls are perfectly elastic, meaning no kinetic energy is lost during the impact.
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