1. In a 100mL sealed flask, 0.1 g of H2 gas reacts with 0.15 g of N2 gas to generate NH3 gas at 25 oC . Note: Consider that i) the initial and final temperatures are 25 oC; ii) all of the limiting reagent is converted to NH3; and iii) the gases behave as ideal. a) Balance the chemical equation :N2(g) + H2(g) ---> NH3(g) b) Calculate the initial pressure inside the flask (before N2 and H2 react). Calculate the initial partial pressures of N2 and H2 (before N2 and H2 react) c) Calculate the final pressure inside the flask (after N2 and H2 react to generate NH3). Calculate the final partial pressures for N2, H2 and NH3 (after N2 and H2 react to generate NH3).
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.
1. In a 100mL sealed flask, 0.1 g of H2 gas reacts with 0.15 g of N2 gas to generate NH3 gas at 25 oC . Note: Consider that i) the initial and final temperatures are 25 oC; ii) all of the limiting reagent is converted to NH3; and iii) the gases behave as ideal.
a) Balance the chemical equation :
N2(g) + H2(g) ---> NH3(g)
b) Calculate the initial pressure inside the flask (before N2 and H2 react). Calculate the initial partial pressures of N2 and H2 (before N2 and H2 react)
c) Calculate the final pressure inside the flask (after N2 and H2 react to generate NH3). Calculate the final partial pressures for N2, H2 and NH3 (after N2 and H2 react to generate NH3).
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