PCl3(g) + Cl2(g) PCl5(g); some PCl5 is removed Ans. ______________ 2 SO3(g) 2 SO2(g) + O2(g); pressure is increased Ans. ______________ COBr2(g) + 18.2 kcal CO(g) + Br2(g); temperature is increased Ans. ______________ 2 NOBr(g) 2 NO(g) + Br2(g); catalyst is added Ans. ______________ 2 NO(g) + Cl2(g) 2 NOCl(g); exothermic; temperature is increased Ans. ______________ BaCO3 (s) BaO(s) + CO2(g); BaO is added Ans. ______________ PCl3(g) + Cl2(g) PCl5(g) + energy; the reaction is cooled
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.
- (2 pts each) The following reactions have been allowed to reach equilibrium. Consider the following changes that are introduced to the system and predict the direction of the equilibrium shift (to the left or to the right). If no equilibrium shift is expected, write "no change".
- PCl3(g) + Cl2(g) PCl5(g); some PCl5 is removed
Ans. ______________
- 2 SO3(g) 2 SO2(g) + O2(g); pressure is increased
Ans. ______________
- COBr2(g) + 18.2 kcal CO(g) + Br2(g); temperature is increased
Ans. ______________
- 2 NOBr(g) 2 NO(g) + Br2(g); catalyst is added
Ans. ______________
- 2 NO(g) + Cl2(g) 2 NOCl(g); exothermic; temperature is increased
Ans. ______________
- BaCO3 (s) BaO(s) + CO2(g); BaO is added
Ans. ______________
- PCl3(g) + Cl2(g) PCl5(g) + energy; the reaction is cooled
Ans. ______________
- HPO42- (aq) + H2O(l) PO43-(aq) + H3O+(aq); NaOH is added
Ans. ______________
- C2H4 (g) + I2 (g) C2H4I2 (g) + heat; a catalyst is added
Ans. ______________
- AgBr (s) Ag+ (aq) + Br- (aq); AgBr is added
Ans. ______________
- (5 points) Use the Henderson-Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 ´ 10–5.
- Buffer A: Calculate the mass of solid sodium acetate required to mix with 100.0 mL of 0.5 M acetic acid to prepare a pH 4 buffer.
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