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Pressure is directly proportional to moles only for ideal gases at constant temperature and volume. The ideal gas law is PV = nRT, where P = pressure, V = volume, n = number of moles, R is a gas constant that depends only on the units being used, and T is temperature (in degrees Kelvin).

Solving for pressure gives P = (RT/V)n.

The ideal gas law is a decent approximation for most cases, but it becomes less accurate for larger molecules and at lower temperatures. That's because it assumes that the gas particles' only interaction is to bounce off each other in perfect elastic collisions. Larger particles tend to "bounce" in more complicated ways, and at lower temperatures the particles are moving slowly enough that intermolecular forces begin to become significant.

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