A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water. Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid. Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal. Refer to Table 1 and calculate the partial pressure of hydrogen gas. Temperature Pressure Temperature Pressure Temperature Pressure 16 °C 14 mm Hg 21 °C 19 mm Hg 26 °C 24 mm Hg 17 °C 15 mm Hg 22 °C 20 mm Hg 27 °C 25 mm Hg 18 °C 16 mm Hg 23 °C 21 mm Hg 28 °C 26 mm Hg 19 °C 17 mm Hg 24 °C 22 mm Hg 29 °C 27 mm Hg 20 °C 18 mm Hg 25 °C 23 mm Hg 30 °C 28 mm Hg Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected.
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 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at 23 oC and an atmospheric pressure of 756 mm Hg. The hydrogen gas is collected over water.
- Write a balanced chemical equation for the reaction between solid aluminum metal and aqueous hydrochloric acid.
- Using stoichiometry, determine the theoretical yield of hydrogen gas (in moles) that will be produced by the complete reaction of the aluminum metal.
- Refer to Table 1 and calculate the partial pressure of hydrogen gas.
|
Temperature |
Pressure |
Temperature |
Pressure |
Temperature |
Pressure |
|
16 °C |
14 mm Hg |
21 °C |
19 mm Hg |
26 °C |
24 mm Hg |
|
17 °C |
15 mm Hg |
22 °C |
20 mm Hg |
27 °C |
25 mm Hg |
|
18 °C |
16 mm Hg |
23 °C |
21 mm Hg |
28 °C |
26 mm Hg |
|
19 °C |
17 mm Hg |
24 °C |
22 mm Hg |
29 °C |
27 mm Hg |
|
20 °C |
18 mm Hg |
25 °C |
23 mm Hg |
30 °C |
28 mm Hg |
- Using the
Ideal Gas Law , determine the experimental moles of hydrogen gas collected.
- Calculate the % yield of the reaction based on the actual yield (d) and the theoretical yield (b) calculations above.
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