Gas pressure

Gas pressure is force per unit area exerted when gas particles collide with a surface. It emerges from the particles’ collective momentum transfer.

Kinetic theory of gases: A model that explains gas properties through the motion and interactions of microscopic particles. It derives pressure from particle momentum transferred to container walls.
Pressure: The normal force exerted per unit area on a surface. Gas pressure is a specific form of this general physical quantity.
Barometer: An instrument that measures atmospheric pressure. A barometer converts the force of gas pressure into a readable measurement.
Partial pressure: The pressure contributed by one gas in a mixture under specified conditions. A mixture’s total gas pressure combines the contributions of its components.
Molecular speed distribution: The statistical distribution of molecular speeds in a gas at a given temperature. Faster molecules transfer more momentum during wall collisions, affecting pressure.
Ideal gas law: An equation relating pressure, volume, amount, and temperature for an ideal gas. It summarizes how gas pressure varies with volume, temperature, and particle amount.
Manometer: An instrument that measures pressure using the height or deformation of a fluid or element. Manometers compare gas pressure with a reference pressure.
Gauge pressure: Pressure measured relative to the surrounding atmospheric pressure. It differs from absolute gas pressure by the local atmospheric reference.
Maxwell–Boltzmann distribution: A probability distribution describing particle speeds in a classical ideal gas at thermal equilibrium. It specifies the spread of molecular speeds behind kinetic pressure predictions.
Temperature: A physical quantity that characterizes thermal state and determines the direction of heat transfer. For a fixed volume and amount, higher temperature raises ideal-gas pressure.

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