What happens to pressure if the container expands? As long as the temperature is constant, the average force of each particle striking the surface will be the same. Because the area of the container has increased, there will be fewer of these collisions per unit area and the pressure will decrease.

Area and force are the two factors on which pressure depend.

For a fixed mass of gas at constant temperature, the volume is inversely proportional to the pressure. That means that, for example, if you double the pressure, you will halve the volume. If you increase the pressure 10 times, the volume will decrease 10 times.

this relationship between pressure and volume is called Boyle’s law. So, at constant temperature, the answer to your answer is: the volume decreases in the same ratio as the ratio of pressure increases. BUT, in general, there is not a single answer to your question. But you won’t get any change in volume.

If the temperature of the gas is doubled and the volume is quadrupled, the pressure becomes half the initial pressure.

V is linear. Figure 6. The relationship between pressure and volume is inversely proportional. Graphically, this relationship is shown by the straight line that results when plotting the inverse of the pressure (1P) versus the volume (V), or the inverse of volume (1V) versus the pressure (V).

Decreasing the volume of a gas increases the pressure of the gas. More collisions mean more force, so the pressure will increase. When the volume decreases, the pressure increases. This shows that the pressure of a gas is inversely proportional to its volume.

Gay-Lussac’s Law or Third Gas Law states that for a constant volume, the pressure is directly proportional to absolute temperature: P alpha T; also stated as P/T = K, where K is a constant, and similarly, P1/T1 = P2/T2.

Diphosphorus

First, let’s review the ideal gas law, PV = nRT. In this equation, ‘P’ is the pressure in atmospheres, ‘V’ is the volume in liters, ‘n’ is the number of particles in moles, ‘T’ is the temperature in Kelvin and ‘R’ is the ideal gas constant (0.0821 liter atmospheres per moles Kelvin).

The units used in the ideal gas equation that PV = nRT are:

• P is pressure measured in Pascals.
• V is the volume measured in m.
• n is the number of moles.
• R is the universal gas constant measured in J/(K. mol)
• T is the temperature measured in Kelvin.