Exercise 2N₂O5(soln) [N₂O5] (mol/L) 4NO₂(soln) + O₂(g) Time (s) 0 200 400 600 800 1000 1200 1400 1600 1800 2000 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 Determine the order of reaction, half-life and rate a. zero order, k=0.0511, half-life-2562.35 b. 2nd order, k-0.0011, half-life-3255.755 c. 1st order, k=0.0006, half-life=1155.245 d. 1st order, k=0.0011, half-life=1155.245 e. 2nd order, k=0.0011, half-life=1155.245
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.
![Exercise
2N₂O5(soln) → 4NO₂(soln) + O₂(g)
Time (s)
0
200
400
600
800
1000
1200
1400
1600
1800
2000
e.
[N₂O5] (mol/L)
1.00
0.88
0.78
0.69
0.61
0.54
0.48
0.43
0.38
0.34
0.30
Determine the order of reaction, half-life and rate constant
a. zero order, k=0.0511, half-life=2562.35
b. 2nd order, k=0.0011, half-life-3255.755
C. 1st order, k=0.0006, half-life=1155.245
d. 1st order, k=0.0011, half-life=1155.245
2nd order, k=0.0011, half-life=1155.245](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F085dc6bd-923d-4464-9877-584eb11cc314%2F95b31e56-dee8-49a5-b457-e82ade8228fa%2F5pydeji_processed.jpeg&w=3840&q=75)
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