One of the components of smog is ozone,O3, a colorless, toxic gas. It is a very strong oxidizing agent and causes respiratory illnesses. Ozone is produced in the lower atmosphere due to the catalytic effect of nitric oxide, NO, a byproduct of the combustion process in car engines. However, in the upper atmosphere ozone is a very useful gas, because it absorbs ultraviolet radiation and protects the earth from this high energy, damaging radiation. It is referred to as the ozone layer. This ozone layer is depleted by the catalytic action of gases like Freon, which are commonly used in refrigerators and air conditioners. Chemically these gases are unreactive and rise into the upper atmosphere. The high energy radiation in the upper atmosphere produces very reactive chlorine atoms according to the reaction below: CCl2F2(g) → CClF2(g) + Cl(g) (catalyzed by uv radiation) The following questions refer to the depletion of ozone in the upper atmosphere according to the mechanism shown below: step 1: Cl(g) + O3(g) → ClO(g) + O2(g) (slow) step 2: O(g) + ClO(g) → Cl(g) + O2(g) (fast) Mark each of the following statements as either True or False: The sum of the two steps is equal to the overall reaction: O(g) + O3(g) → 2O2(g). The rate law is deduced directly from the coefficients of the overall reaction. Cl(g) is a catalyst in this reaction mechanism. ClO(g) is an intermediate formed in this reaction mechanism. The rate equation for this mechanism is rate = k [O][ClO]. Step 2 of the mechanism is a bimolecular.
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.
One of the components of smog is ozone,O3, a colorless, toxic gas. It is a very strong oxidizing agent and causes respiratory illnesses. Ozone is produced in the lower atmosphere due to the catalytic effect of nitric oxide, NO, a byproduct of the combustion process in car engines.
However, in the upper atmosphere ozone is a very useful gas, because it absorbs ultraviolet radiation and protects the earth from this high energy, damaging radiation. It is referred to as the ozone layer. This ozone layer is depleted by the catalytic action of gases like Freon, which are commonly used in refrigerators and air conditioners. Chemically these gases are unreactive and rise into the upper atmosphere. The high energy radiation in the upper atmosphere produces very reactive chlorine atoms according to the reaction below:
CCl2F2(g) → CClF2(g) + Cl(g) (catalyzed by uv radiation)
The following questions refer to the depletion of ozone in the upper atmosphere according to the mechanism shown below:
| step 1: | Cl(g) + O3(g) | → | ClO(g) + O2(g) | (slow) |
| step 2: | O(g) + ClO(g) | → | Cl(g) + O2(g) | (fast) |
Mark each of the following statements as either True or False:
The sum of the two steps is equal to the overall reaction: O(g) + O3(g) → 2O2(g).
The rate law is deduced directly from the coefficients of the overall reaction.
Cl(g) is a catalyst in this reaction mechanism.
ClO(g) is an intermediate formed in this reaction mechanism.
The rate equation for this mechanism is rate = k [O][ClO].
Step 2 of the mechanism is a bimolecular.
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