What is the relationship between the pressure and volume of a gas?
Follow
 ✓Follow publicly
 ✓Follow privately
 Unfollow
Describe the relationship between the pressure and volume of a gas.
Best Answer
In general, the relationship between pressure and volume of a gas is unknown and must be determined experimentally. However, a large number of real gases can be modeled as ideal gases. The basic assumption behind the ideal gas model is that individual molecules of the gas do not interact. The ideal gas equation of state is given as
PV=nRT
where P is pressure, V is volume, n is number of particles, R is the ideal gas constant, and T is temperature. Knowing something about the number of particles and the temperature can yield an expression relating P and V. For example, for a closed system (n is constant) at constant temperature (T is constant), we have
PV=constant
which is commonly known as Boyle's Law. Another relationship between P and V for an ideal gas which is more complex is for an isentropic process where
P*V^gamma=constant
where gamma is the specific heat ratio.
PV=nRT
where P is pressure, V is volume, n is number of particles, R is the ideal gas constant, and T is temperature. Knowing something about the number of particles and the temperature can yield an expression relating P and V. For example, for a closed system (n is constant) at constant temperature (T is constant), we have
PV=constant
which is commonly known as Boyle's Law. Another relationship between P and V for an ideal gas which is more complex is for an isentropic process where
P*V^gamma=constant
where gamma is the specific heat ratio.
Other Answers (6)
Rated Highest
They are inversely proportional. As pressure increases volume will decrease. For more specifics look up Boyle's law.

Boyle's Law... At a constant temperature the volume of a given mass of gas is inversely proportional to its pressure.

Boyle's lawnamed for Robert Boylestates that, at constant temperature, the pressure P of a gas varies inversely with its volume V, or PV = k, where k is a constant.
Charles's lawnamed for J.A.C. Charles (1746–1823)states that, at constant pressure, the volume V of a gas is directly proportional to its absolute (Kelvin) temperature T, or V/T = k.
These two laws can be combined to form a single generalization of the behaviour of gases known as an equation of state,
PV = nRT,
where n is the number of grammoles of a gas and R is called the universal gas constant. Though this law describes the behaviour of an ideal gas, it closely approximates the behaviour of real gases.Source(s):

If you reduce the volume by 1/2 you double the pressure after the temperature is reduced to where you started. I mean absolute pressure, not gage pressure. in other words the relationship is directly proportional, but you have to consider absolute temperature also. like 101 compression at sea level after cooling back is147 psi

mathematical relationship: PV = nRT
P = pressure (atmospheres)
V = volume (Liters)
n = # of moles
R = constant (0.08206)
T = temperature (Kelvin)
This equation is called the ideal gas law. You can see from it that when pressure goes UP, volume should go DOWN and vice versa. Hence, they are inversely proportional 
As pressure increases, volume decreases
( or as gas is being squeezed it is being force into a tighter space )
Sign In
to add your answer
Ask a Question
Discover Questions