Pressure is inversely proportional to:

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When evaluating how pressure relates to other variables in a gas, we must consider the conditions that keep the relationship simple and well-defined.
Option 1: Gas Constant. The gas constant R is a proportionality constant that appears in the ideal gas law PV = nRT, but pressure itself is not inversely proportional to R; R is a constant depending on units, not a variable that pressure inversely tracks.
Option 2: Volume. Under conditions of fixed amount of gas, fixed temperature, and constant number of particles, pressure varies inversely with volume as described by Boyle's law: as volume increases, pressure decreases, and as volume decreases, pressure increases. This inverse relation is the classic, textbook example of P ∝ 1/V.
Option 3: Number of particles. If you increase the number of particles at fixed volume and temperature, pressure tends to rise because more collisions occur with container walls. That is a direct, not inverse, relationship in the typical ideal-gas framework.
Option 4: Temperature. Temperature is directly related to pressure when volume and amount of gas are held constant (Gay-Lussac's law): higher temperature leads to higher pressure due to increased molecular kinetic energy and more forceful wall collisions. Again, this is a direct relation, not inverse.
In sum, only volume yields an inverse dependence with pressure in the standard condition set, while the other options either stay constant, increase pressure directly with the variable, or involve a constant that does not itself vary to produce an inverse relation.

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Pressure is inversely proportional to:

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