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n/V is concentration, therefore this equation can also be seen as P=(concentration)RT or P/RT=(concentration). This allows us to convert from concentration to pressure or pressure to concentration in case a problem gives us some equilibrium information as pressure or some as concentration.
As far as I've seen, the ideal gas law is taught in high school chemistry classes more than physics classes, but that's a bit of a moot point. That said, could we possibly use other variants of the law to figure things out as well, such as P(mm) = dRT (where mm = molar mass and d = density)?
You can use this equation to find partial pressures of the components of the reaction (P) if you know the volume, temperature and molar concentration. Then you could find the equilibrium constant Kp by plugging in the partial pressures into the formula for Kp.
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