gas syringe

(noun)

An item of laboratory equipment used to withdraw a volume of gas from a closed chemical system for measurement and/or analysis.

Related Terms

Examples of gas syringe in the following topics:

  • Measuring Reaction Rates

    • The volume of oxygen produced can be measured using the gas syringe method.
    • The gas collects in the syringe, pushing out against the plunger.
    • The volume of gas that has been produced can be read from the markings on the syringe.
    • The rate of a reaction that produces a gas can also be measured by calculating the mass loss as the gas forms and escapes from the reaction flask.
    • In a reaction that produces a gas, the volume of the gas produced can be measured using the gas syringe method.

  • Pneumothorax and Hemothorax

    • Pneumothorax, or collapsed lung, is an abnormal collection of air or gas in the pleural space of the lung that interferes with breathing.
    • A pneumothorax is an abnormal collection of air or gas in the pleural space that separates the lungs from the chest wall, which may interfere with normal breathing .
    • In larger pneumothoraces, or when there are marked signs and/or symptoms, the air may be extracted with a syringe or a chest tube connected to a one-way valve system.

  • Filtration

    • A syringe filter with a pore size of 0.22 micrometers, small enough to capture and retain bacterial and fungal cells.

  • Equations of State

    • The ideal gas law is the equation of state of a hypothetical ideal gas (in which there is no molecule to molecule interaction).
    • The ideal gas law is the equation of state of a hypothetical ideal gas (an illustration is offered in ).
    • while Charles' law states that volume of a gas is proportional to the absolute temperature T of the gas at constant pressure
    • The proportionality factor is the universal gas constant, R, i.e.
    • Therefore, we derive a microscopic version of the ideal gas law

  • Gas Vesicles

    • There is a simple relationship between the diameter of the gas vesicle and pressure at which it will collapse - the wider the gas vesicle the weaker it becomes.
    • However, wider gas vesicles are more efficient.
    • They provide more buoyancy per unit of protein than narrow gas vesicles.
    • This will select for species with narrower, stronger gas vesicles.
    • Discuss the role of a gas vesicle in regards to survival

  • Density Calculations

    • The Ideal Gas Equation in the form $PV=nRT$ is an excellent tool for understanding the relationship between the pressure, volume, amount, and temperature of an ideal gas in a defined environment that can be controlled for constant volume.
    • We know the Ideal Gas Equation in the form $PV=nRT$.
    • The term $\frac{m}{V}$ appears on the right-hand side of the above rearranged Ideal Gas Law.
    • This derivation of the Ideal Gas Equation allows us to characterize the relationship between the pressure, density, and temperature of the gas sample independent of the volume the gas occupies; it also allows us to determine the density of a gas sample given its pressure and temperature, or determine the molar mass of a gas sample given its density.
    • Atmospheric science offers one plausible real-life application of the density form of the ideal gas equation.

  • Molar Mass of Gas

    • We can derive a form of the Ideal Gas Equation, PV=nRT, that incorporates the molar mass of the gas (M, $g*mol^{-1}$ ).
    • The molar mass of an ideal gas can be determined using yet another derivation of the Ideal Gas Law: $PV=nRT$.
    • We can plug this into the Ideal Gas Equation:
    • This derivation of the Ideal Gas Equation is useful in determining the molar mass of an unknown gas.
    • What is the molar mass of the gas?

  • Constant Pressure

    • For an ideal gas, this means the volume of a gas is proportional to its temperature (historically, this is called Charles' law).
    • Therefore, the work done by the gas (W) is:
    • Using the ideal gas law PV=NkT (P=const),
    • Here n is the amount of particles in a gas represented in moles.
    • $c_P = \frac{5}{2} kN_A = \frac{5}{2} R$ for a monatomic gas.

  • The Effect of the Finite Volume

    • Real gases deviate from the ideal gas law due to the finite volume occupied by individual gas particles.
    • The ideal gas law is commonly used to model the behavior of gas-phase reactions.
    • At high pressures where the volume occupied by gas molecules does not approach zero
    • The particles of a real gas do, in fact, occupy a finite, measurable volume.
    • The available volume is now represented as $V - nb$, where b is a constant that is specific to each gas.

  • Expressing the Equilibrium Constant of a Gas in Terms of Pressure

    • Take the general gas-phase reaction:
    • Recall that the ideal gas law is given by:
    • In this expression, $\Delta n$ is a measure of the change in number of moles of gas in the reaction.
    • For instance, if a reaction produces three moles of gas, and consumes two moles of gas, then $\Delta n=(3-2)=1$.
    • Write the equilibrium expression, KP, in terms of the partial pressures of a gas-phase reaction