# Considering the ideal gas law PV = nRT, what is P directly proportional to?

Here's what's going on here.

First, confirm that you truly understand what is meant by directly proportional.

Two quantities must either increase as the other increases or decrease as the other decreases, both at the same rate, for them to be considered directly proportional.

Let's start with the number of moles. You must maintain the other two variables constant in order to determine whether there is direct or inverse proportionality.

As long as the temperature and volume remain constant, the number of moles and the pressure are exactly equal.

It can be stated that once more, a rise in temperature will lead to an increase in pressure, and a fall in temperature will lead to a decrease in pressure.

According to Gay Lussac's Law, pressure and temperature are directly correlated when the number of moles and volume are held constant.

Lastly, maintain a constant temperature and mole count while observing the effects of volume variation on pressure.

Since volume is now in the denominator, a rise in volume would cause a drop in pressure this time.

Thus, when the number of moles and temperature are held constant, pressure is not directly proportional to volume. Conversely, a decrease in volume would lead to an increase in pressure.

Nonetheless, you could say that

Boyle's Law states that when temperature and the number of moles are held constant, pressure is inversely proportional to volume.

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Pressure (P) is directly proportional to temperature (T) when volume (V), amount of substance (n), and the gas constant (R) are held constant.

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