A 5.0-L flask contains a mixture of ammonia and nitrogenat 27°C and a total pressure of 3.00 atm. The sample ofgas is allowed to flow from the flask until the pressure inthe flask has fallen to 1.00 atm. The gas that escapes ispassed through 1.50 L of 0.200 M acetic acid. All theammonia in the gas that escapes is absorbed by the solution and turns out to be just sufficient to neutralize theacetic acid present. The volume of the solution does notchange significantly.(a) Will the electrical conductivity of the aqueous solution change significantly as the gas is absorbed? Give equations for any reactions, and calculate the final concentrations of the principal ions present (if any) at the end.(b) Calculate the percentage by mass of ammonia in the flask initially.
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
A 5.0-L flask contains a mixture of ammonia and nitrogen
at 27°C and a total pressure of 3.00 atm. The sample of
gas is allowed to flow from the flask until the pressure in
the flask has fallen to 1.00 atm. The gas that escapes is
passed through 1.50 L of 0.200 M acetic acid. All the
ammonia in the gas that escapes is absorbed by the solution and turns out to be just sufficient to neutralize the
acetic acid present. The volume of the solution does not
change significantly.
(a) Will the electrical conductivity of the aqueous solution change significantly as the gas is absorbed? Give
equations for any reactions, and calculate the final
concentrations of the principal ions present (if any) at
the end.
(b) Calculate the percentage by mass of ammonia in the
flask initially.
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