Equilibrium
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7.40. Classify the following species into Lewis acids and Lewis bases and show how these can act as Lewis acid/Lewis base?
(a) OH– (b) F– (c) H+ (d) BCl3
7.40. Classify the following species into Lewis acids and Lewis bases and show how these can act as Lewis acid/Lewis base?
(a) OH– (b) F– (c) H+ (d) BCl3
(a) OH– ions can donate an electron pair and act as Lewis base.
(b) F– ions can donate an electron pair and actas Lewis base.
(c) H+ ions can accept an electron pair and act as Lewis acid.
(d) BCl3 can accept an electron pair since Boron atom is electron deficient. It
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<p><strong>7.39. The species H<sub>2</sub>O, HCO<sub>3</sub><sup>–</sup>, HSO<sub>4</sub><sup>–</sup> and NH<sub>3</sub> can act both as Bronsted acid and base. For each case, give the corresponding conjugate acid and base. </strong></p>
7.38. Write the conjugate acids for the following Bronsted bases:
NH2, NH3 and HCOO–
7.38. Write the conjugate acids for the following Bronsted bases:
NH2, NH3 and HCOO–
7.37. What will be the conjugate bases for the Bronsted acids: HF, H2SO4 and H2CO3?
7.37. What will be the conjugate bases for the Bronsted acids: HF, H2SO4 and H2CO3?
7.36. Which of the following are Lewis Acids?
H2O,BF3, H+ and NH4+
7.36. Which of the following are Lewis Acids?
H2O,BF3, H+ and NH4+
7.35. What is meant by conjugate acid-base pair? Find the conjugate acid/base for the following species: HNO2, CN–, HClO4F–, OH–, CO32-, and S2-.
7.35. What is meant by conjugate acid-base pair? Find the conjugate acid/base for the following species: HNO2, CN–, HClO4F–, OH–, CO32-, and S2-.
An acid-base pair which differs by a proton only is known as conjugate acid-base pair. For example, HCl, and Cl represents conjugate acid base pair.
The conjugate acid/base for the species HNO2, CN–, HClO4F–, OH–, CO32-, and S2- are NO2–, HCN, ClO4–, HF, H2O, HCO3– and HS–.respectively.
Upvote 7.34. The reaction, CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) is at equilibrium at 1300 K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H2 and 0.02 mol of H2O and an unknown amount of CH4 in the flask. Determine the concentration of CH4 in the mixture. The equilibrium constant, Kc for the reaction at the given temperature is 3.90.
7.34. The reaction, CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) is at equilibrium at 1300 K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H2 and 0.02 mol of H2O and an unknown amount of CH4 in the flask. Determine the concentration of CH4 in the mixture. The equilibrium constant, Kc for the reaction at the given temperature is 3.90.
Kc = [CH4] [H2O] / [CO] [H2]3
3.90 = [CH4]×0.02 / (0.30) (0.10)3
[CH4] = 3.90×0.30× (0.10)3 / 0.02
=5.85×102 M
Thus, the concentration of methane in the mixture is 5.85×102 M.
Upvote 7.33. The value of Kc for the reaction 3O2(g) ⇌2O3(g) is 2.0 x 10-50 at 25°C. If equilibrium concentration of O2 in air at 25°C is 1.6 x 10-2, what is the concentration of O3?
7.33. The value of Kc for the reaction 3O2(g) ⇌2O3(g) is 2.0 x 10-50 at 25°C. If equilibrium concentration of O2 in air at 25°C is 1.6 x 10-2, what is the concentration of O3?
The equilibrium constant expression is
Kc = [O3]2 / [O2]3
2.0×1050 = [O3]2 / (1.6×102)3
[O3]2=2.0×1050× (1.6×102)3
=8.192×1056
Hence, the equilibrium concentration of ozone is
[O3]= 2.86×1028M
Upvote 7.32. Predict which of the following will have appreciable concentration of reactants and products:
a) Cl2 (g) ⇌2Cl (g) Kc = 5 ×10–39
b) Cl2 (g) + 2NO (g) ⇌2NOCl (g) Kc = 3.7 × 108
c) Cl2 (g) + 2NO2 (g) ⇌2NO2Cl (g) Kc = 1.8
7.32. Predict which of the following will have appreciable concentration of reactants and products:
a) Cl2 (g) ⇌2Cl (g) Kc = 5 ×10–39
b) Cl2 (g) + 2NO (g) ⇌2NOCl (g) Kc = 3.7 × 108
c) Cl2 (g) + 2NO2 (g) ⇌2NO2Cl (g) Kc = 1.8
Following conclusions can be drawn from the values of Kc .
(a) Since the value of Kc is very small, this means that the molar concentration of the products is very small as compared to that of the reactants.
(b) Since the value of Kc is quite large, this means that the molar concentra
Upvote 7.31. Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high temperature steam. The first stage of two stage reaction involves the formation of CO and H2 In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction.
CO (g) + H2O(g) ⇌ CO2(g) + H2(g)
If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam so that PCO = PH2O = 4.0 bar, what will be the partial pressure of H2 at equilibrium? Kp = 10.1 at 400°C.
7.31. Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high temperature steam. The first stage of two stage reaction involves the formation of CO and H2 In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction.
CO (g) + H2O(g) ⇌ CO2(g) + H2(g)
If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam so that PCO = PH2O = 4.0 bar, what will be the partial pressure of H2 at equilibrium? Kp = 10.1 at 400°C.
Let the partial pressures of CO and H2 be p.
CO (g) + H2?O(g) ? CO2?(g) + H2?(g)
Initial conc. 4 bar 4 bar &nb
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