Gas Pressure Volume
Gas Pressure Volume - Related Videos
02:32
Le Chatelier's Principle: Changing Volume (Pressure)
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2020
For gas-phase equilibria, changes in the concentrations of reactants and products can occur with altered volume and pressure. The partial pressure, P, of an ideal gas is proportional to its molar concentration, M. So changes in the partial pressures of any reactant or product are essentially changes in concentrations; therefore, these changes yield the same effects on equilibria. Aside from adding or removing reactants or products, the pressures (concentrations) of species in a gas-phase...
03:43
Applications of the Ideal Gas Law: Molar Mass, Density, and Volume
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2020
The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT, suggests that the volume of a given quantity of gas and the number of moles in a given volume of gas vary with changes in pressure and temperature. At standard temperature and pressure, or STP (273.15 K and 1 atm), one mole of an ideal gas (regardless of its identity) has a volume of about 22.4 L — this is referred to as the standard molar volume. For example, one mole each of hydrogen, oxygen,...
09:49
Measurement of the Pressure-volume Curve in Mouse Lungs
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Cited by 47 •
2015
Here we present a protocol to simply and reliably measure the lung pressure-volume curve in mice, showing that it is sufficiently sensitive to detect phenotypic parenchymal changes in two common lung pathologies, pulmonary fibrosis and emphysema. This metric provides a means to quantify the lung’s structural changes with developing pathology.
09:15
Measuring Pressure Volume Loops in the Mouse
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Cited by 16 •
2016
This manuscript describes a detailed protocol for the collection of pressure-volume data from the mouse.
08:54
Measuring Blood Pressure in Mice using Volume Pressure Recording, a Tail-cuff Method
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Cited by 175 •
2009
The CODA 8-Channel High Throughput Non-Invasive Blood Pressure system measures the blood pressure in up to 8 mice or rats simultaneously. This tail-cuff system uses Volume Pressure Recording (VPR) to measure the blood pressure by determining the tail blood volume.
FAQs
At the particle level, compression does not create more gas particles; it gives the existing particles less space. They therefore reach and collide with the container walls more frequently, producing a higher pressure. Expansion has the opposite effect, with fewer wall collisions over a given interval. This collision pattern explains the inverse pressure-volume trend.
Boyle’s law isolates the effect of volume by keeping temperature and the amount of gas constant. If either condition changes, the observed pressure shift may reflect more than the change in available space. Controlling both variables therefore makes the pressure-volume relationship interpretable and allows comparisons between measurements to test the expected inverse pattern.
Because pressure and volume are inversely proportional under the stated conditions, a measured change in one property can be used to calculate the other. The relationship is commonly represented by a constant pressure-volume product for a fixed gas sample. Comparing calculated values across measurements helps determine whether the data follow Boyle’s law.
A useful investigation records pressure and volume for the same amount of gas while temperature remains constant. Measurements can then be compared as paired values, and the pressure-volume product or inverse trend can be examined. Agreement across trials supports the expected relationship; disagreement signals that the controlled conditions or measurements should be reconsidered.
In a syringe, pump, or respiratory system, changing the available volume changes how often gas particles strike the surrounding surfaces when temperature and gas amount are controlled. Reducing space corresponds to more frequent collisions and higher pressure, whereas increasing space corresponds to lower pressure. This gives a chemistry-based framework for understanding their operation.
The pressure-volume relationship provides a foundation for interpreting gas laws because it links a measurable mechanical change, volume, with a measurable response, pressure. Chemists can use that link to predict how a gas responds to physical changes and to organize observations from compression, expansion, and experiments involving compressible gases without treating pressure or volume as isolated properties.