At 330.0 K, nitrogen monoxide and hydrogen react to form nitrogen gas and water vapour as below; 2 NO(g) + 2 H2(g) →N2{g) + 2 H¿O{g) Experiment shows that the rate constant for the reaction is 2.88 x 10 M's' and the rate of reaction is only depending on the concentration of NO. The total pressure of the products formed is 1.20 atm. [R=0.0821 Latm/molK] (a) Calculate the time (minutes) required for 25% of the NO to react. (b) State the factor by which the rate of reaction change if the concentrations of both reactants are doubled. (c) Calculate the partial pressure and the density of nitrogen gas produced.
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.
this is the full question, it is for my own revision and it is not graded. i'll be having a chemistry exam this wednesday ? please don't reject the question if it's possible to answer. based on the answer scheme given by my lecturer, the partial pressure is 0.4 atm and the density is 0.414 g/L.
![At 330.0 K, nitrogen monoxide and hydrogen react to form nitrogen gas and water vapour as below;
2 NO(g) + 2 H2(g) →N2{g) + 2 H¿O(g)
Experiment shows that the rate constant for the reaction is 2.88 x 10 M's' and the rate of reaction is only
depending on the concentration of NO. The total pressure of the products formed is 1.20 atm.
[R=0.0821 Latm/molK]
(a) Calculate the time (minutes) required for 25% of the NO to react.
(b) State the factor by which the rate of reaction change if the concentrations of both reactants are doubled.
(c) Calculate the partial pressure and the density of nitrogen gas produced.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F453b2fb0-289a-45e5-a97f-cc442700ead2%2F18ddd230-ce61-459c-86c3-5fba0852b70b%2Fysyeo3n_processed.png&w=3840&q=75)
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