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Gas law calculations

The ideal gas law can be used to solve a variety of problems. We will show how you can use it to find— [Pg.107]

A gas commonly undergoes a change from an initial to a final state. Typically, you are asked to determine the effect on V, P, n, or T of a change in one or more of these variables. For example, starting with a sample of gas at 25°C and 1.00 atm, you might be asked to calculate the pressure developed when the sample is heated to 95°C at constant volume. [Pg.108]

The ideal gas law is readily applied to problems of this type. A relationship between the variables involved is derived from this law. In this case, pressure and temperature change, while n and V remain constant. [Pg.108]

To obtain a two-point equation, write the gas law twice and divide to eliminate constants. [Pg.108]

Dividing the second equation by the first cancels V, n, and R, leaving the relation [Pg.108]

A common calculation is that of the volume of a gas, starting with a particular volume and changing temperature and/or pressure. This kind of calculation follows logically from the ideal gas equation, but can also be reasoned out, knowing that an increase in temperature causes an increase in volume, whereas an increase in pressure causes a decrease in volume. Therefore, a second volume, Vj is calculated from an initial volume, Vj, by the relationship [Pg.59]

The use of this relationship in doing gas law calculations requires only that one remember the following  [Pg.60]

When the temperature of a quantity of gas changes while the pressure stays the same, the resulting calculation is a Charles law calculation. As an example of such a calculation, calculate the volume of a gas with an initial volume of 10.0 L when the temperature changes from -11.0°C to 95.0°C at constant pressure. The first step in solving any gas law problem involving a temperature change is to convert Celsius temperatures to kelvin  [Pg.60]

Note that in this calculation, it is seen that the temperature increases this increases the volume, so the higher temperature is placed over the lower. Furthermore, since Fj = Fj, the factor for the pressure ratio simply drops out. [Pg.60]

Calculate next the volume of a gas with an initial volume of 10.0 L after the temperature decreases from 111.0°C to 2.0°C at constant pressure  [Pg.60]


Typically, in gas law calculations, temperatures are expressed only to the nearest degree. In that case, the Kelvin temperature can be found by simply adding 273 to the Celsius temperature. [Pg.103]

Remember In any gas law calculation, you must express the temperature in kelvin. [Pg.106]

A—The average kinetic energy of the molecules depends on the temperature. The correct answer involves a temperature difference (333 K— 303 K). Do not forget that ALL gas law calculations require Kelvin temperatures. [Pg.118]

Absolute temperatures, the Kelvin scale, must be used when performing gas law calculations. [Pg.67]

Assume this laser pulse is completely absorbed by a black wall. Use the relation E = cp to calculate the momentum it transfers to the wall. By analogy with the calculations we did to derive the ideal gas law, calculate the radiation pressure the pulse exerts on the 10 /rm spot while it is on. [Pg.172]

I The units must be the same on each side of the equation in all gas law calculations. [Pg.357]

One part of. xenon (0.361 g 0.00275 mol) is condensed into the reaction vessel F by means of liquid nitrogen. The quantity of xenon is best measured by the pressure, according to gas law calculations based on the known volume of the vessel F,... [Pg.256]

Remember from Chapter 11 that the most convenient unit for counting numbers of atoms or molecules is the mole. One mole contains 6.02 X 10 particles. The molar volume for a gas is the volume that one mole occupies at 0.00°C and 1.00 atm pressure. These conditions of temperature and pressure are known as standard temperature and pressure (STP). Avogadro showed experimentally that one mole of any gas will occupy a volume of 22.4 L at STP. The fact that this value is the same for all gases greatly simplifies many gas law calculations. Because the volume of one mole of a gas at STP is 22.4 L, you can use the following conversion factor to find the number of moles, the mass, and even the number of particles in a gas sample. [Pg.431]

First, he would have to convert °C to Kelvin, because the gas law calculations aren t based on the Celsius scale. [Pg.226]

The Ideal Gas Law can be used when any one of the four variables is missing, provided the other information is known. R, which is a constant, is the same for every calculation. The units that come with the constant, R, dictate the units that we must have for the other quantities for the calculation. For example, we must work in Kelvin for temperature and kilopascals for pressure. If we were asked to do a problem with atmospheres of pressure or Celsius degrees for temperature, we would need to make a conversion before we performed our Ideal Gas Law calculation. [Pg.281]

When the gaseous products are simple and can be readily predicted from the composition of the reactant, e.g. nitrogen from metal azides or oxygen from metal permanganates, it may be possible to determine the overall stoichiometry from simple gas-law calculations from pressures of gas collected under calibrated conditions. Even such systems, however, may yield atomic or ionic, rather than molecular, species as intermediates [76] and these require more specific methods of detection. [Pg.62]

The reader is cautioned on the use of acfm and/or scfm (see Problem THR.5). Predicting the performance and the design of equipment should always be based on actual conditions. Designs based on standard conditions can lead to disastrous results, with the unit usually underdesigned. For example, the ratio of acfm (2140°F) to scfm (60°F) for a particular application is 5.0. The reader is again reminded that absolute temperatures and pressures must be employed in all ideal gas law calculations. [Pg.152]

The units of R that are appropriate for ideal gas law calculations are those that involve units of volume, pressure, moles, and temperature. When you use the value R = 0.0821 L atm/mol K, remember to express all quantities in a calculation in these units. Pressures should be expressed in atmospheres, volumes in liters, temperature in kelvins, and amount of gas in moles. In Examples 12-9 and 12-10 we converted pressures from torr to atm. In Example 12-10 the volume was converted from ft to L. [Pg.452]

Standard electrode potentials, designated refer to standard-state conditions. These standard-state conditions are one molar solutions for ions, one atmosphere pressure for gases, and all solids and liquids in their standard states at 25°C. (Remember that we refer to thermodynamic standard-state conditions, and not standard temperature and pressure as in gas law calculations.) As any of the standard cells described earlier operates, and concentrations or pressures of reactants change, the observed cell voltage drops. Similarly, cells constructed with solution concentrations different from one molar, or gas pressures different from one atmosphere, cause the corresponding potentials to deviate from standard electrode potentials. [Pg.877]

Absolute zero (-273.15°C) is the lowest theoretically attainable temperature. The Kelvin temperature scale takes 0 K as absolute zero. In aU gas law calculations, temperature must be expressed in kelvins. [Pg.190]

The combined gas law provides a convenient expression for performing gas law calculations involving the most common variables pressure, volume, and temperature. [Pg.169]


See other pages where Gas law calculations is mentioned: [Pg.102]    [Pg.107]    [Pg.107]    [Pg.109]    [Pg.126]    [Pg.354]    [Pg.417]    [Pg.452]    [Pg.73]    [Pg.74]    [Pg.75]    [Pg.76]    [Pg.77]    [Pg.78]    [Pg.79]    [Pg.80]    [Pg.81]    [Pg.82]    [Pg.83]    [Pg.84]    [Pg.64]    [Pg.597]    [Pg.354]    [Pg.447]    [Pg.447]    [Pg.448]    [Pg.447]    [Pg.447]    [Pg.448]   
See also in sourсe #XX -- [ Pg.125 , Pg.126 , Pg.127 , Pg.128 , Pg.129 , Pg.130 ]




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