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Concentration is moles per unit volume, which is the same as (n/V). If you rearrange the ideal gas law (PV=nRT) with this in mind, you'll see that pressure is directly proportional to concentration; in other words, as concentration increases, so does pressure.
The relationship stated above is correct. In addition, if you think of the situation of pressure and concentration conceptually, it makes sense as well. If the amount of moles of a molecule in the volume container (with a constant temperature) increases, the pressure of the gas increases. This is because there is an increase in the amount or frequency of collisions between the gas molecules, thereby exerting a greater amount of pressure on the container.
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