Mass of a Gas

SORT The problem gives you the temperature and pressure of a gas and asks you to find its density. The problem states that the gas is nitrogen. [Pg.211]

STRATEGIZE Equation 5.6 provides the relationship between the density of a gas and its temperature, pressure, and molar mass. The temperature and pressure are given. You can calculate the molar mass from the formula of the gas, which we know is N2. [Pg.211]

SOLVE To solve the problem, gather each of the required quantities in the correct units. Convert the temperature to kelvins and the pressure to atmospheres. [Pg.211]

Substitute the quantities into the equation to calculate density. [Pg.211]

CHECK The units of the answer are correct. The magnitude of the answer (0.852 g/L) makes sense because earlier we calculated the density of nitrogen gas at STP as 1.25 g/L. Since the temperature is higher than standard temperature, it follows that the density is lower. [Pg.211]

The continuity equation is a mathematical formulation of the law of conservation of mass of a gas that is a continuum. The law of conservation of mass states that the mass of a volume moving with the fluid remains unchanged... [Pg.117]

Assuming no flow losses occur, the total mass of a gas introduced into and out of the system must be constant. Hence,... [Pg.735]

Henry s law States that the mass of a gas dissolved in a definite volume of liquid at constant temperature is proportional to the partial pressure of the gas. [Pg.1447]

The ideal gas law offers a simple approach to the experimental determination of the molar mass of a gas. Indeed, this approach can be applied to volatile liquids like acetone (Example 5.4). All you need to know is the mass of a sample confined to a container of fixed volume at a particular temperature and pressure. [Pg.109]

The state of unit mass of a gas, like that of any other fluid, is defined by any pair of the variables p, r, 0, and its characteristic equation is therefore ... [Pg.131]

We see that, for a given pressure and temperature, the greater the molar mass of the gas, the greater its density. Equation 10 also shows that, at constant temperature, the density of a gas increases with pressure. When a gas is compressed, its density increases because the same number of molecules are confined in a smaller volume. Similarly, heating a gas that is free to expand at constant pressure increases the volume occupied by the gas and therefore reduces its density. The effect of temperature on density is the principle behind hot-air balloons the hot air inside the envelope of the balloon has a lower density than that of the surrounding cool air. Equation 10 is also the basis for using density measurements to determine the molar mass of a gas or vapor. [Pg.274]

EXAMPLE 4.6 Sample exercise Calculating the molar mass of a gas from its density... [Pg.274]

It can be assumed that the gas mixture follows ideal gas behavior and that the kilogram molar mass of a gas occupies 22.4 m3 at standard conditions of 0°C and 1 atm (1.013 bar)... [Pg.192]

However, suppose that you have forgotten the convenient formula for the density of an ideal gas You can still solve a problem such as this one. The density of 1.00 g/L indicates a mass of 1.00 g of gas in a 1.00-L volume. Of course, the mass of a gas, given its identity (oxygen in this case) enables us to determine the amount in moles of the gas (n in the ideal gas equation). Then, we can solve the ideal gas equation for the desired property, such as temperature, as follows ... [Pg.106]

Previous studies of Vapor Cloud Explosions (VCE) have used a correlation between the mass of a gas in the cloud and equivalent mass of TNT to predict explosion overpressures. This was always thought to give conservative results, but recent research evidence indicates that this approach is not accurate to natural gas and air mixtures. The TNT models do not correlate well in the areas near to the point of ignition, and generally over estimate the level of overpressures in the near field. Experiments on methane explosions in "unconfined" areas have indicated a maximum overpressure of 0.2 bar (2.9 psio). This overpressure then decays with distance Therefore newer computer models have been generated to better simulate the effects... [Pg.50]

Background The Ideal Gas Law can be used to determine the approximate molecular mass of a gas through the equation MM = t y. In this experiment, a small amount of a volatile liquid is placed into a flask (of which you know the volume) and allowed to vaporize. A small pinhole in the system allows the pressure of the gas to equalize with the air pressure. The temperature of the vapor will be assumed to be the temperature of the boiling water in which the flask is immersed. At this point, you know g, R, T, V, and R You will then be able to calculate the apparent MM. [Pg.259]

An experiment to determine the molecular mass of a gas begins by heating a solid to produce a gaseous product. The gas passes through a tube and displaces water in an inverted, water-filled bottle. Which of the following necessary items may be determined after the experiment is completed ... [Pg.114]

Graham s law—The lower the molecular mass of a gas, the faster it will effuse/diffuse. [Pg.121]

The ideal gas law is a powerful tool that the chemist—and now you—can use to determine the molar mass of an unknown gas. By measuring the temperature, pressure, volume, and mass of a gas sample, you can calculate the molar mass of the gas. [Pg.54]

What is the molecular mass of a gas that diffuses through a porous membrane 1.86 times faster than Xe What might the gas be ... [Pg.375]

Demonstrate the ammonia and hydrochloric acid experiment described in the text (Figure 1.14, p. 7). This also illustrates the dependence of the rate of diffusion on the relative molecular mass of a gas, Mr... [Pg.263]

From the graph obtained, what relationship exists between the molar mass of a gas and its boiling point ... [Pg.461]

The molar mass of a gas refers to the mass (in g) of one mole of the gas. You can calculate molar mass by adding the masses of atoms in the periodic table. You can also calculate molar mass by dividing the mass of a sample by the number of moles that are present. Molar mass is always expressed in the units g/mol. Table 12.2 summarizes molar volume, density, and molar mass. [Pg.490]

If the mass of a gas is tripled and the pressure is quadrupled while the temperature is constant, by what factor will the volume of the gas change ... [Pg.651]

At constant temperature the volume occupied by a definite mass of a gas is inversely proportional to the applied pressure. [Pg.8]

One last way to express concentration is the column abundance, which is the total amount or mass of a gas within a vertical column of air above a specific location. Column abundances have units of amount per area (i.e., mol m-2, kg m-2). In the particular case of stratospheric ozone, data are... [Pg.72]

The molar mass of a gas may be calculated if the mass of a sample and the number of moles of the sample are both known. The ideal gas law may be used to determine the number of moles, from which the molar mass may be calculated. As introduced in Section 7.4, the molar mass, along with the empirical formula, may then be used to determine the molecular formula (Section 12.7). [Pg.357]

The Ideal Gas Equation -Calculating the Mass and Relative Molecular Mass of a Gas... [Pg.182]

What is the molar mass of a gas if it diffuses 0.907 times the speed of... [Pg.456]

Estimate the molar mass of a gas that effuses at 1.60 times the effusion rate of carbon dioxide. [Pg.887]

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