(a) [COCI2] = 2.00 × 10-³ M, [CO]= 3.3 × 10-6 M, [Cl2] = 6.62 × 10-6 M %3D %3D 15.7 (b) [COCI2] = 4.50 × 10-² M, [CO] = 1.1 × 10-7 M, [Cl2] = 2.25 x 10-6 M %3D %3D (c) [COCI2] = 0.0100 M, [CO] = [Cl2] = 1.48 × 10-6 M %3D bon 15.44 As shown in Table 15.2, K, for the equilibrium N2(8) + 3 H2(g) = 2 NH3(g) is 4.51 X 10-5 at 450 °C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 °C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. (a) 98 atm NH3, 45 atm N2, 55 atm H2 (b) 57 atm NH3, 143 atm N2, no H2 (c) 13 atm NH3, 27 atm N2, 82 atm H2 15.45 At 100 °C, K. = 0.078 for the reaction %3D SO,Cl2(8) = SO2(g) + Cl2(8) In an equilibrium mixture of the three gases, the con- centrations of SO2C12 and SO, are 0.108 M and 0.052 M, respectively. What is the partial pressure of Cl2 in the equi- librium mixture? 15.46 At 900 K, the following reaction has K, = 0.345: 2 SO2(g) + O2(g) = 2 SO3(g) In an equilibrium mixture the partial pressures of SO2 and O are 0.135 atm and 0.455 atm, respectively. What is the librium partial pressure of SO3 in the mixture? equi
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question 15.44
![(a) [COCI2] = 2.00 × 10-³ M, [CO]= 3.3 × 10-6 M,
[Cl2] = 6.62 × 10-6 M
%3D
%3D
15.7
(b) [COCI2] = 4.50 × 10-² M, [CO] = 1.1 × 10-7 M,
[Cl2] = 2.25 x 10-6 M
%3D
%3D
(c) [COCI2] = 0.0100 M, [CO] = [Cl2] = 1.48 × 10-6 M
%3D
bon
15.44 As shown in Table 15.2, K, for the equilibrium
N2(8) + 3 H2(g) = 2 NH3(g)
is 4.51 X 10-5 at 450 °C. For each of the mixtures listed
here, indicate whether the mixture is at equilibrium at
450 °C. If it is not at equilibrium, indicate the direction
(toward product or toward reactants) in which the mixture
must shift to achieve equilibrium.
(a) 98 atm NH3, 45 atm N2, 55 atm H2
(b) 57 atm NH3, 143 atm N2, no H2
(c) 13 atm NH3, 27 atm N2, 82 atm H2
15.45 At 100 °C, K. = 0.078 for the reaction
%3D
SO,Cl2(8) = SO2(g) + Cl2(8)
In an equilibrium mixture of the three gases, the con-
centrations of SO2C12 and SO, are 0.108 M and 0.052 M,
respectively. What is the partial pressure of Cl2 in the equi-
librium mixture?
15.46 At 900 K, the following reaction has K, = 0.345:
2 SO2(g) + O2(g) = 2 SO3(g)
In an equilibrium mixture the partial pressures of SO2 and O
are 0.135 atm and 0.455 atm, respectively. What is the
librium partial pressure of SO3 in the mixture?
equi](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2f71cc3-406d-4549-a751-96d454552a8c%2Fee396741-b271-4cef-a16a-a854143eb628%2F0on7o9.jpeg&w=3840&q=75)
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